The molar enthalpy for the reaction 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g) is 266.4 kJ/mol.
What is the molar enthalpy for the reaction?The molar enthalpy is determined from Hess's law as follows:
Equation 1 x2:
2 N₂ (g) + 2 O₂ (g) → 4 NO (g) ∆H° = 361.2 kJ/mol
Equation 3 x3, :
6 H₂ (g) + 3 O₂ (g) → 6 H₂O (g) ∆H° = -1451.1 kJ/mol
Equation 2 x -4:
-8 N₂ (g) - 12 H₂ (g) → -8 NH₃ (g) ∆H° = 367.2 kJ/mol
Adding the equations together:
-6 N₂ (g) - 6 H₂ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g) - 8 NH₃ (g) ∆H° = 266.3 kJ/mol
Multiplying the equation above by -1/2:
3 N₂ (g) + 3 H₂ (g) - 5/2 O₂ (g) → -2 NO (g) - 3 H₂O (g) + 4 NH₃ (g) ∆H° = -133.2 kJ/mol
Multiplying the above equation by -2:
4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g) ∆H° = 266.4 kJ/mol
This is the molar enthalpy of the given reaction
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What is the electron configuration for magnesium (Mg)?
O A. 1s²2s²2p²356
B. 15²25²3s23p6
C. 3s²3p 3d
D. 1s²2s²2p63s²
Answer:
D is correct.(1s22s22p63s2)
diagram of reaction of water,oxygen,acids
When water and oxygen react in the presence of an acid, the oxygen can oxidize the acid to produce a compound and release hydrogen ions.
Reaction:
The reaction is as follows and it's diagram mentioned below.
Acid + Oxygen + Water → Compound + Hydrogen ions
if we take the acid hydrochloric acid (HCl), the reaction with oxygen and water can produce the compound chlorine dioxide ([tex]ClO_{2}[/tex]) and hydrogen ions ([tex]H^{+}[/tex]):
2 HCl + [tex]O_{2}[/tex] + [tex]H_{2}O[/tex] → 2 [tex]ClO_{2}[/tex] + 4 [tex]H^{+}[/tex]
This type of reaction is known as an oxidation-reduction reaction or a redox reaction, where one species is oxidized (loses electrons) while the other is reduced (gains electrons).
What is redox reaction?
A redox reaction, also known as an oxidation-reduction reaction, is a type of chemical reaction in which there is a transfer of electrons between two species. One species undergoes oxidation, meaning it loses electrons, while the other species undergoes reduction, meaning it gains electrons.
Redox reactions are fundamental to many processes in nature and technology, including photosynthesis, respiration, corrosion, and energy production in batteries and fuel cells. They are also important in many industrial processes, such as the production of metals, chemicals, and pharmaceuticals.
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Does anyone have Personal Care services on E2020
Here are some questions on Personal Care services on E2020 are:
A client with a new ileostomy has been home for four days. The HHA is giving the client a bath and notices that the pouch is full. The HHA should say to the client: D. "I'll empty the pouch for you."A client is bedridden at home and has an infected draining sacral wound. The infection control supplies that should be kept in the home is: Gloves.What is infection?An infection is the entrance and growth of dangerous microorganisms in the body that harm the host, such as bacteria, viruses, fungus, or parasites.
Infections can be systemic (affecting the entire body) or localized (affecting a particular area of the body), and they can be moderate to severe.
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The change in enthalpy (AH, ) for a reaction is -25.8 kJ mol.
The equilibrium constant for the reaction is 1.4 × 103 at 298 K.
What is the equilibrium constant for the reaction at 655 K?
The equilibrium constant for the reaction at 655 K is [tex]e^{6.96}[/tex] ≈ 1.05 × 10^3.
The equilibrium constant (K) for a reaction is related to the change in Gibbs free energy (ΔG) through the equation:
ΔG = -RTlnK
where R is the gas constant, T is the temperature in kelvin, and ln is the natural logarithm. Since ΔG and ΔH (the change in enthalpy) are related by the equation:
ΔG = ΔH - TΔS
where ΔS is the change in entropy, we can rearrange the first equation to get:
lnK = -ΔH ÷ RT + ΔS ÷ R
At 298 K, we can use the given values of ΔH and K to solve for ΔS:
lnK = -ΔH ÷ RT + ΔS ÷ R
ln(1.4 × 10³) = (-(-25.8 × 10³ J/mol) ÷ (8.314 J/mol K × 298 K)) + ΔS ÷ 8.314 J/mol K
ΔS = 78.2 J/mol K
Now we can use the equation above to solve for lnK at 655 K, using the same value of ΔH and the newly calculated value of ΔS:
lnK = -ΔH ÷ RT + ΔS ÷ R
lnK = -(-25.8 × 10³ J/mol) ÷ (8.314 J/mol K × 655 K) + (78.2 J/mol K) ÷ 8.314 J/mol K
lnK = 6.96
e ≈ 1.05 × 10³
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Iron pyrite (FeS2) is the form in which much of
the sulfur exists in coal. In the combustion of
coal, oxygen reacts with iron pyrite to produce
iron(III) oxide and sulfur dioxide, which is a
major source of air pollution and a substantial
contributor to acid rain. What mass of Fe2O3
is produced from 74 L of oxygen at 2.97 atm
and 161◦C with an excess of iron pyrite?
Answer in units of g
The mass of Fe₂O₃ produced is 101.9 g.
How to calculate mass ?The balanced chemical equation for the combustion of iron pyrite is:
4FeS₂(s) + 11O₂(g) → 2Fe₂O3(s) + 8SO₂(g)
From the equation, 11 moles of oxygen are required to produce 2 moles of Fe₂O₃. Convert the given volume of oxygen to moles:
n(O2) = PV/RT = (2.97 atm)(74 L)/(0.0821 L·atm/mol·K)(161 + 273 K) = 3.51 mol
Since the reaction requires 11 moles of O₂ for every 2 moles of Fe₂O₃, calculate the moles of Fe₂O₃ produced:
n(Fe₂O₃) = (2/11) × n(O₂) = (2/11) × 3.51 mol = 0.638 mol
Finally, use the molar mass of Fe₂O₃ to convert moles to grams:
m(Fe₂O₃) = n(Fe₂O₃) × M(Fe₂O₃) = 0.638 mol × 159.69 g/mol = 101.9 g
Therefore, the mass of Fe₂O₃ produced is 101.9 g.
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What will happen when pressure on a reactant mixture at equilibrium and with fewer moles on the reactant side is increased
when pressure of the reactant mixture at the equilibrium and with the fewer moles in reactant side will be increased and the equilibrium will be shift to the side in the reaction where the fewer moles of the gas.
According to the Le Chartelier, when the reaction is in the equilibrium phase and the one of the constraints which will affect the rate of the reactions, and the equilibrium will be shift to the cancel out this effect that the constraint had.
Therefore, If the pressure of the system or the reaction is in the equilibrium is change, the equilibrium of the reaction will be change that is depending on the side of the reaction with the highest number of the molecules.
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Describe the intermolecular forces that must be overcome to convert each of the following from a liquid or solid to a gas.
P2O5 and HI
For P₂O₅ the intermolecular forces such as van der Waals forces, dipole-dipole interactions, and hydrogen bonding must be overcome.
For HI the intermolecular forces that must be overcome are as van der Waals forces, dipole-dipole interactions, and hydrogen bonding.
What are the intermolecular forces that must be overcome?P₂O₅ is a covalent compound and it is solid. To convert P₂O₅ from a solid to a gas, intermolecular forces such as van der Waals forces, dipole-dipole interactions, and hydrogen bonding must be overcome.
HI is a covalent compound that is a gas at room temperature and pressure. To convert HI from a liquid to a gas, intermolecular forces such as van der Waals forces, dipole-dipole interactions, and hydrogen bonding must be overcome.
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What is the family puzzle worksheet answer? Please make the pedigree and give me the answers
Interpreting Data:
Joshua's parents must be heterozygous carriers for cystic fibrosis (Nn).Bella's parents must be homozygous for the normal allele (NN).How to analyze family pedigrees?Predicting:
Joshua's brother has a 50% chance of being a carrier for cystic fibrosis (Nn) and a 50% chance of having the normal genotype (NN). This is because Joshua's parents are both carriers, so each of their children has a 50% chance of inheriting the recessive allele.
Communicating:
As a genetic counselor, information about many generations of a family is needed to draw conclusions about a hereditary condition because traits are passed down from generation to generation. By studying the family history, we can identify patterns of inheritance and determine the likelihood that a person has inherited a certain trait. This information can help us make informed decisions about genetic testing and treatment options.
Additionally, knowing the family history can help us determine the risk of passing on a genetic condition to future generations.
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Image transcribed and complete question:
Family Puzzle
Problem
A husband and wife want to understand the probability that their children might inherit cystic fibrosis. How can you use the information in the labeled Case Study to predict the probability?
Skills Focus
interpreting data, predicting
Materials
12 index cards
scissors marker
Procedure
1. Read the Case Study. In your notebook, draw a pedigree that shows all the family members. Use circles to represent the females, and squares to represent the males. Shade in the circles or squares representing the individuals who have cystic fibrosis.
2. You know that cystic fibrosis is controlled by a recessive allele. To help you figure out Joshua and Bella's family pattern, create a set of cards to represent the alleles. Cut each of six index cards into four smaller cards. On 12 of the small cards, write N to represent the dominant normal allele. On the other 12 small cards, write n for the recessive allele.
Case Study:
Joshua and Bella
• Joshua and Bella have a son named lan. lan has been diagnosed with cystic fibrosis.
⚫ Joshua and Bella are both healthy.
• Bella's parents are both healthy.
• Joshua's parents are both healthy. • Joshua's sister, Sara, has cystic fibrosis.
Analyze and Conclude
Write your answers in the spaces provided.
1. Interpreting Data What were the genotypes of Joshua's parents? What were the genotypes of Bella's parents?
2. Predicting Joshua also has a brother. What is the probability that he has cystic fibrosis? Explain.
3. Communicating Imagine that you are a genetic counselor. A couple asks why you need information about many generations of their families to draw conclusions about a hereditary condition. Write an explanation you can give to them.
More to Explore
Review the pedigree that you just studied. What data suggest that the traits are not sex-linked? Explain.
If a balloon containing a mixture of gases where the partial pressure of oxygen is 12.8 psi, the partial pressure of hydrogen is 4.31 psi, and the partial pressure of nitrogen is 22.1 psi, then the actual pressure inside the balloon is…
Answer:
39.21 psi
Explanation:
According to Dalton's Law, the total pressure in the system is the sum of all the partial pressures, so all you need to do is add the partial pressures :)
A titration setup was used to determine the unknown molar concentration of a solution of NaOH. A1.2 M HCl solution was used as the
titration standard. The following data were collected.
Trial 1
Amount of HCI
Standard Used 10.0 mL
0.0 mL
Initial NaOH
Buret Reading
Final NaOH
Buret Reading 12.2 mL
Trial 2
10.0 mL
12.2 mL
23.2 mL
Trial 3 Trial 4
10.0 mL 10.0 mL
23.2 mL 35.2 mL
35.2 mL 47.7 mL
79) Calculate the volume of NaOH solution used to neutralize 10.0 ml. of the standard HCl solution in trial 3 in the given diagram.
[Show your work.]
The enthalpy combustion of ethanol is -1430 kJ/mol. Determine heat given off from the combustion of 1 dm³ of ethanol. Given density of ethanol is 0.79 gcm³. (molar mass ethanol = 46 g/mol)
Answer:
The enthalpy of combustion of ethanol is -1430 kJ/mol, which means that for every mole of ethanol that is burned, 1430 kJ of heat is released.
To determine the amount of heat given off from the combustion of 1 dm³ of ethanol, we need to first calculate the number of moles of ethanol in 1 dm³.
1 dm³ is equivalent to 1000 cm³. Since the density of ethanol is 0.79 g/cm³, the mass of 1 dm³ of ethanol can be calculated as:
mass = density x volume
mass = 0.79 g/cm³ x 1000 cm³
mass = 790 g
To convert this mass to moles, we need to divide by the molar mass of ethanol:
moles = mass / molar mass
moles = 790 g / 46 g/mol
moles = 17.17 mol
Therefore, 1 dm³ of ethanol contains 17.17 moles of ethanol.
To calculate the heat given off from the combustion of 1 dm³ of ethanol, we can use the following equation:
heat = enthalpy of combustion x moles of ethanol
heat = -1430 kJ/mol x 17.17 mol
heat = -24,551 kJ
Therefore, the heat given off from the combustion of 1 dm³ of ethanol is -24,551 kJ, or approximately 24,551 kJ of heat is released.
draw the lewis structure of ch3br
The Lewis structure of the compound[tex]CH_{3} Br[/tex] is shown in the image attached.
What is the Lewis structure?The Lewis structure of a molecule or ion is produced by arranging the atoms in a manner that lessens the attraction between their valence electron pairs and then distributes the valence electrons among the atoms to form covalent bonds.
The octet rule, which states that atoms normally gain or lose electrons to obtain a stable configuration with eight valence electrons, frequently serves as a guidance when arranging electrons in the Lewis structure.
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A sample of gas is contained in a 245 mL flask at a temperature of 23.5°C. The gas pressure is 37.8 mm Hg. The gas is moved to a new flask, which is then immersed in ice water, and which has a volume of 54 mL. What is the pressure of the gas in the smaller flask at the new temperature?
We can use the combined gas law to solve this problem:
(P1V1/T1) = (P2V2/T2)
where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 are the final pressure, volume, and temperature, respectively.
We are given that the initial pressure is P1 = 37.8 mm Hg and the initial volume is V1 = 245 mL. The initial temperature is T1 = 23.5°C, which we need to convert to Kelvin by adding 273.15:
T1 = 23.5°C + 273.15 = 296.65 K
We are also given that the final volume is V2 = 54 mL, and the final temperature is the temperature of the ice water, which is 0°C or 273.15 K.
Now we can solve for the final pressure, P2:
(P1V1/T1) = (P2V2/T2)
P2 = (P1V1T2) / (V2T1)
P2 = (37.8 mm Hg * 245 mL * 273.15 K) / (54 mL * 296.65 K)
P2 = 24.4 mm Hg
Therefore, the pressure of the gas in the smaller flask at the new temperature is 24.4 mm Hg.
A solution has [H+] = 1.39x10^-6 M. What is the pH?
Answer:
the pH of the solution is approximately 5.857.
Explanation:
The pH of a solution can be calculated using the formula:
pH = -log[H+]
where [H+] is the concentration of hydrogen ions in moles per liter (M).
In this case, [H+] = 1.39x10^-6 M, so:
pH = -log(1.39x10^-6)
= 5.857
Therefore, the pH of the solution is approximately 5.857.
We wish to determine the mass of Mg required to react completely with 250mL of 1.0 M HCI. HCI reacts with Mg according to the equation below.
2HCl(aq) + Mg(s) → MgCl₂(aq) + H₂(g)
How many moles of HCI are present in 250. mL of 1.0 M HCl?
There are 0.25 moles of HCl present in 250 mL of 1.0 M HCl.
We have to calculate the number of moles of HCl present in some mL of 1.0M HCl. A mole is defined as the amount of substance in a system that contains as many elementary entities as there are atoms in 0.012 kg of carbon 12. We represent mole by the symbol 'mol'. Now, we will see how to calculate the number of moles.
We can calculate the number of moles of a substance using the following expression;
Molarity = no of moles of an element/volume
According to this question, we were given 250. mL of 1.0 M HCl. The number of moles will be calculated by the formula as follows;
no of moles of HCl = 0.250L × 1.0M
no of moles of HCl = 0.250 moles.
Therefore, 0.25 moles are present in 250 mL of 1.0 M HCl.
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A solution of thickness 3cm transmits 30%. calculate the concentration of the solution. E= 400dm/mol/cm
The concentration of the solution is 0.000435 mol/dm³.
What is the concentration of the solution?The concentration of a solution is calculated as follows;
Concentration = (Absorbance) / (Molar absorptivity x path length)
the path length = 3cm
the molar absorptivity (E) = 400 dm/mol/cm.
if the solution transmits 30% of the light, it absorbs 70% of the incident light.
Absorbance = log (1/Transmittance)
Absorbance = log (1/0.3)
Absorbance = 0.523
Concentration = (0.523) / (400 dm/mol/cm x 3 cm)
= 0.000435 mol/dm³
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How many grams of NiNO can be produced if 35.1 g of ammonium nitrate and 552 g of sodium phosphate react?
Answer:its b
Explanation:
jusut bcss
For the reaction:
S8(s) + 8 O2(g)⟶8 SO2(g) ΔH = –2368 kJ
How much heat is evolved when 25.0 moles of sulfur is burned in excess oxygen?
The amount of heat evolved when 25 moles of Sulfur is burned in excess oxygen is -74000 kJ.
The balanced reaction is given that is:
[tex]S_8(s) + 8 O_2(g) \rightarrow 8 SO_2(g)[/tex]
We can see that 1 mole of [tex]S_8[/tex] reacts with 8 moles of [tex]O_2[/tex] to produce 8 moles of [tex]So_2[/tex].
If 25.0 moles of [tex]S_8[/tex] reacts with excess Oxygen, then the amount of [tex]O_2[/tex] which is required in the reaction will be:
8 moles [tex]O_2[/tex] / 1 mole S8 × 25.0 moles S8 = 200 moles [tex]O_2[/tex]
We can use the enthalpy change and calculate the amount of heat evolved:
[tex]\Delta H[/tex] = -2368 kJ/ 8 moles [tex]SO_2[/tex]
The heat evolved = [tex]\Delta H[/tex] × moles of [tex]SO_2[/tex] produced
Moles of [tex]SO_2[/tex] produced = 8 moles [tex]SO_2[/tex] / 1 mole [tex]S_8[/tex] × 25.0 moles [tex]S_8[/tex]
= 200 moles [tex]SO_2[/tex].
Therefore, Heat evolved= -2368 kJ/ 8 moles [tex]SO_2[/tex] × 200 moles [tex]SO_2[/tex]
= -74000 kJ
The amount of heat evolved when 25 moles of Sulfur is burned in excess oxygen is -74000 kJ, the negative sign here indicates that the reaction is exothermic.
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determine the solubility of NH and 90° C
The solubility of NH₃ in water at 90°C is approximately 0.03 g per 100 g of water.
What is the solubility of NH₃?The solubility can be determined from a solubility table or by using the appropriate equilibrium constant.
According to a solubility table, the solubility of ammonia in water at 90°C is approximately 88 g per 100 g of water.
Alternatively, the equilibrium constant for the dissolution of ammonia in water at 90°C can be used to calculate the solubility.
The equilibrium constant (K) for the reaction:
NH3 (g) + H2O (l) ⇌ NH4+ (aq) + OH- (aq)
is approximately 1.76 x 10⁻⁵ at 90°C.
Using the equilibrium constant expression:
K = [NH4+][OH-]/[NH3][H2O]
Assuming that the concentration of water remains constant at 100 g per 100 g of solution, and that the concentration of NH4+ and OH- are negligible compared to that of NH3, the solubility of NH3 can be calculated as:
[NH3] = K[H2O] = 1.76 x 10⁻⁵ x 100 = 1.76 x 10⁻³ mol/L
Converting to grams per 100 g of water:
1.76 x 10⁻³ mol/L x 17.03 g/mol = 0.03 g/100 g of water
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The complete question is below:
determine the solubility of NH₃ in water at 90° C
a student mixed 20 grams of salt into a beaker with 200 milliliters of warm water. then, the student set the cup of saltwater on a windowsill undisturbed for one week. what changes did the student observe? include what happened when salt was mixed with warm water and what most likely happened to the saltwater after one week.
Answer:
Water molecules pull the sodium and chloride ions apart, breaking the ionic bond that held them together. After the salt compounds are pulled apart, the sodium and chloride atoms are surrounded by water molecules, as this diagram shows. Once this happens, the salt is dissolved, resulting in a homogeneous solution.
Explanation:
Given Equation (Balance it) :
C2H4O2 + NaHCO3 —> NaC2H3O2 + H2O + CO2
Word Problem:
If you have 100 mg of Acetic Acid (C2H4O2) and 10 mg of NaHCO3 (Sodium Bicarbonate), how many grams of CO2 can be produced ?
also determine the theoretical yield of the chemical reaction.
C₂H₄O₂ + NaHCO₃ —> NaC₂H₃O₂ + H₂O + CO₂ the amount of Carbon dioxide produced is 5.28 mg.
Is the reaction between acetic acid and sodium bicarbonate exothermic or endothermic?Water, CO₂ , and C₂H₃NaO₂ were produced when acetic acid and NaHCO₃ were combined. The chemistry is as follows: The reaction between vinegar and baking soda was endothermic.
Acetic acid: 2(12.01 g/mol) + 4(1.01 g/mol) + 2(16.00 g/mol)
= 60.05 g/mol
NaHCO₃ 22.99 g/mol + 1.01 g/mol + 3(16.00 g/mol)
= 84.01 g/mol
100 mg of Acetic acid is equal to 0.1 g, and 10 mg of NaHCO₃ is equal to 0.01 g.
Number of moles of Acetic acid = 0.1 g / 60.05 g/mol
= 0.00167 mol
Number of moles of NaHCO₃ = 0.01 g / 84.01 g/mol
= 0.00012 mol
Since NaHCO₃ has fewer moles, it is the limiting reactant.
Therefore, 0.00012 mol of NaHCO₃ will produce 0.00012 mol of CO₂
The mass of CO₂ produced can be calculated as follows:
Mass of CO₂ = Number of moles of CO₂ x Molar mass of CO₂
Mass of CO₂ = 0.00012 mol x 44.01 g/mol
= 0.00528 g or 5.28 mg
Therefore, the amount of CO₂ produced is 5.28 mg.
The theoretical yield of CO₂ is 0.00012 mol x 44.01 g/mol
= 0.00528 g or 5.28 mg.
This is equal to the actual yield of CO₂ produced.
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Explain how your model is different from the model in the picture.
My model is distinct from the model in the image in that it takes a more thorough and all-encompassing approach to comprehending the fundamental parts of a system.
It considers the interactions between various system elements as well as the connections between those elements and their surroundings. It also looks at how the system changes over time, and how different components interact with each other.
As a result, the system may be understood more precisely, and management choices can be made with more knowledge. In order to offer a more precise and current picture of the system, my model also integrates the most recent research and technological advancements.
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6. A 90.0 gram sample of an unknown solid is heated to 80 °C and placed into a calorimeter containing 120 grams of water at 24 °C. If the final temperature of the solid sample and the water is 32 °C, what is the specific heat of solid?
PLEASE SHOW WORK
Answer:
1.02 J/g°C.
Explanation:
We can use the equation:
q = m * c * ΔT
where q is the heat absorbed or released, m is the mass of the substance (in grams), c is the specific heat, and ΔT is the change in temperature (in Celsius).
First, we can calculate the heat gained by the water:
q_water = m_water * c_water * ΔT_water
where m_water is the mass of the water (in grams), c_water is the specific heat of water (4.184 J/g°C), and ΔT_water is the change in temperature of the water.
m_water = 120 g
c_water = 4.184 J/g°C
ΔT_water = (32°C - 24°C) = 8°C
q_water = (120 g) * (4.184 J/g°C) * (8°C) = 4009 J
This means that the heat lost by the unknown solid is equal to the heat gained by the water:
q_solid = -q_water
q_solid = -4009 J
Next, we can calculate the change in temperature of the solid:
ΔT_solid = (32°C - 80°C) = -48°C
Now, we can solve for the specific heat of the solid:
q_solid = m_solid * c_solid * ΔT_solid
-4009 J = (90.0 g) * c_solid * (-48°C)
c_solid = -4009 J / (90.0 g * -48°C)
c_solid = 1.02 J/g°C
Therefore, the specific heat of the unknown solid is 1.02 J/g°C.
How does the frequency of a string affect its wavelength?
Answer:
as the frequency goes down, the speed goes down by the same factor, and so the wavelength doesn't change.
Explanation:
Answer: as the frequency goes down, the speed goes down by the same factor, and so the wavelength doesn't change.
Explanation:
An argon ion laser emits visible radiation with photons of energy 4.071 x 10-19 J. What is the
wavelength of the radiation?
The wavelength of the radiation emitted by the argon ion laser is [tex]4.854 * 10^-7 m[/tex].
Wavelength is a property of any type of wave that refers to the distance between two adjacent points on the wave that is in phase, i.e., at the same point in their respective cycles. It is usually denoted by the Greek letter lambda (λ) and is measured in units of length, such as meters or nanometers.
The energy carried by the photon (E) is related to the wavelength ([tex]\lambda[/tex]) through the following equation:
[tex]E=hc/\lambda[/tex]; where 'h' is the Plank's Constant and 'c' is the speed of light which is [tex]3* 10^{-7} m/s[/tex].
We can say that
[tex]\lambda - hc/E[/tex]
Now after substituting the given values, we get:
[tex]\lambda = (6.626 * 10^{-34} J.s * 3.00 * 10^8 m/s) / (4.071 * 10^{-19} J)\\\lambda = 4.854 * 10^-7 m[/tex]
Therefore the wavelength of the radiation emitted by the argon ion laser is [tex]4.854 * 10^-7 m[/tex].
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Silver chloride, AgCl, is a sparingly soluble solid. Answer the following questions about a saturated solution prepared by placing solid silver chloride in a 2.45 10-5 M NaCl(aq) solution. At some temperature, the silver ion concentration, [Ag+], was found to be 5.36 10-6 M.
(a) What is the concentration of chloride ions, [Cl − ], in the resulting solution?
The solubility of silver chloride (AgCl) can be represented by the following equilibrium equation:
AgCl(s) ⇌ Ag+(aq) + Cl-(aq)
In a saturated solution of AgCl, the concentration of Ag+ ions is equal to the solubility product constant (Ksp) for AgCl at that temperature. Since the concentration of Ag+ ions in the solution is given as 5.36 x 10^-6 M, we can write:
[Ag+] = 5.36 x 10^-6 M
According to the stoichiometry of the equilibrium equation, the concentration of chloride ions ([Cl-]) is also equal to the concentration of Ag+ ions, as one mole of AgCl dissociates to yield one mole of Ag+ ions and one mole of Cl- ions. Therefore:
[Cl-] = 5.36 x 10^-6 M
So, the concentration of chloride ions in the resulting solution is 5.36 x 10^-6 M.
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A 7.95 L
container holds a mixture of two gases at 25 °C.
The partial pressures of gas A and gas B, respectively, are 0.352 atm
and 0.715 atm.
If 0.240 mol
of a third gas is added with no change in volume or temperature, what will the total pressure become?
Why are leaves green
Answer:
Leaves are green due to the presence of an organelle chloroplast (in abundance) which contains the pigment chlorophyll
Explanation:
Now saying chlorophyll pigment is a green pigment might be slightly incorrect. The two famous types (Chlorophyll a, Chlorophyll b) only absorb red and blue light from the atmosphere and reflect green light hence giving the pigment a green appearance and lastly giving the leaves a green color too
Answer:
Chlorophyll
Explanation:
Plants are often seen as green to the human eye due to the presence of chlorophyll, which is the primary pigment used in photosynthesis. Chlorophyll absorbs light in the red and blue-violet parts of the spectrum, but reflects or transmits green light, resulting in the characteristic green color of leaves.
Find the concentration of all ions present in a 0.223 M solution of PbCl2.
Answer:
Since that means that we have 0.223 moles of PbCl2 in 1000mL of solution.
Also since mole ratio of the ions Pb2+:Cl- is 1:2
Thus, moles of Pb2+ = 0.223moles
concentration of Pb2+= 0.223M
Moles of Cl- = 2x0.223 moles
Concentration of Cl- = 0.446M
Explanation:
1. While doing a calorimetry experiment, you notice the temperature of 50.0 g of water changes by 7ºC. What is the energy of the chemical reaction? (Cwater= 4.18 J/g*°C)
2. Which of the following is an example of a kinetic energy change?