**Calculating Equilibrium Constants**The equilibrium constant, \( K \), of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium.For a gaseous reaction with the general form:\[ aA + bB \rightleftharpoons cC + dD \]the \( K_c \) and \( K_p \) expressions are given by:\[ K_c = \frac{{[C]^c[D]^d}}{{[A]^a[B]^b}} \]\[ K_p = \frac{{(P_C)^c(P_D)^d}}{{(P_A)^a(P_B)^b}} \]The subscript c or p indicates whether \( K \) is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved since their composition does not change throughout the reaction. The standard state of a pure substance is the pure substance itself, and although the quantity may change, the sample remains pure. The constant value is incorporated into the value of \( K \), and does not need to be accounted for separately.---### Part APhosgene (carbonyl chloride), \( \text{COCl}_2 \), is an extremely toxic gas used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures:\[ \text{CO}(g) + \text{Cl}_2(g) \rightleftharpoons \text{COCl}_2(g) \]Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at \( 452 \, ^\circ \text{C} \). At equilibrium, the concentrations were measured and the following results obtained:| Gas | Partial Pressure (atm) ||-------|------------------------|| CO | 0.900 || \( \text{Cl}_2 \) | 1.30 || \( \text{COCl}_2 \) | 0.120 |What is the equilibrium constant, \( K_p \), of this reaction?Express your answer numerically.[View Available Hint(s)]\( K_p = \)---(There is also an interactive input box to enter the \( K_p \) value, accompanied by options to format the text and a submit button.) **Understanding Equilibrium Constants**The equilibrium constant, \( K \), of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium.**For a gaseous reaction with the general form:**\[ aA + bB \rightleftharpoons cC + dD \]**The expressions for \( K_c \) and \( K_p \) are:**\[ K_c = \frac{[C]^c[D]^d}{[A]^a[B]^b} \]\[ K_p = \frac{(P_C)^c(P_D)^d}{(P_A)^a(P_B)^b} \]Here, the subscript \( c \) or \( p \) indicates whether \( K \) is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include terms for pure solids or liquids, as their composition does not change throughout the reaction. The standard state of a pure substance is itself, although the quantity may change. The constant value is incorporated into \( K \) and does not need separate accounting.---**Deriving Concentrations from Data**In Part A, equilibrium pressures were provided and could be used directly in the formula for \( K \). However, in Part B, you will be given initial concentrations and only one equilibrium concentration. Use this data to find all three equilibrium concentrations before applying the formula for \( K \).**Part B**A reaction was conducted in a sealed vessel at 740°C:\[ \text{H}_2(g) + \text{I}_2(g) \rightleftharpoons 2\text{HI}(g) \]* Initial concentrations: \([H_2] = 3.00 \, M\) and \([I_2] = 2.15 \, M\)* Equilibrium concentration of \([I_2]\) is 0.0700 \( M \).**Task**Calculate the equilibrium constant, \( K_c \), for the reaction at this temperature. Provide your answer numerically.

Answered: Image /qna-images/answer/9a4c22e8-127f-4da6-994a-a0a299387dbb.jpg

Part A Phosgene (carbonyl chloride), COCI₂, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g) + Cl₂(g) = COC1₂(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 452 °C. At equilibrium, the concentrations were measured and the following results obtained: What is the equilibrium constant, Kp. of this reaction? Express your answer numerically. ▸ View Available Hint(s) Kp = Submit ΨΕ ΑΣΦΑ → Previous Answers Gas CO Cl₂ | COC, BO ? Partial Pressure (atm) 0.900 1.30 0.120

Part A Phosgene (carbonyl chloride), COCI₂, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g) + Cl₂(g) = COC1₂(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 452 °C. At equilibrium, the concentrations were measured and the following results obtained: What is the equilibrium constant, Kp. of this reaction? Express your answer numerically. ▸ View Available Hint(s) Kp = Submit ΨΕ ΑΣΦΑ → Previous Answers Gas CO Cl₂ | COC, BO ? Partial Pressure (atm) 0.900 1.30 0.120

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(g)→ 3 NO,(g)+H,0(1) At a certain temperature, a chemist finds that a 4.5 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount dlo HNO3 14.2 g 18 Ar NO 7.3 g NO, 19.2 g H,O 87.0 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 x10 ?
Iron(III) oxide and hydrogen react to form iron and water, like this: Fe,0;(s)+3 H,(g)→2FE(s)+3H,O(9) At a certain temperature, a chemist finds that a 5.1 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount db Fe,O3 4.36 g H, 4.35 g Fe 3.23 g H,0 2.73 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. Explanation Check 2022 McGraw H LLC. A Rights Reserved Terms of Use Pvacy Center Accessibil DE P Type here to search JU P. Alt alexa ENADLED
Consider the reaction: P(s) + 3/2Cl₂ (g) → PC13 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: P(s) + 5/2Cl₂ (g) ⇒ PCl5(9) K₁ PC13 (g) + Cl2 (g) PC15 (9) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter K² if the first equilibrium constant should be squared. K =
Calcium oxide and carbon dioxide react to form calcium carbonate, like this: CaO(s)+CO,(g)→CaCO3(s) At a certain temperature, a chemist finds that a 8.1 L reaction vessel containing a mixture of calcium oxide, carbon dioxide, and calcium carbonate at equilibrium has the following composition: compound amount СаО 43.8 g CO2 40.9 g CaCO3 55.4 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0 x10
Hydrogen gas and bromine gas are mixed in a sealed container at 250°C and allowed to reach equilibrium. H2(g) + Br2(g) = 2HB1(g) The equilibrium constant for this reaction at 250°C is 65.5. At equilibrium, the concentration of H2 is 0.0510 mol L*1 and the concentration of Brris 0.174 mol L-1 at 250°C. (i) Write the equilibrium constant expression for the above reaction. (ii) Calculate the concentration of HBr in the equilibrium mixture at 250°C (iii) Explain what happens to the concentration of HBr you calculated in (ii) above if the pressure of the equilibrium mixture is increased.
A mixture of 0.578 moles of carbon monoxide and 0.443 moles of oxygen was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium at a certain temperature. The equilibrium concentration of CO2 was 0.239 M. What is the value of Ke for this reaction at this particular temperature? CO(g) + O2(g) = CO2(g) Report your answer to three significant figures and do not include units.
Mercury(II) oxide decomposes to form mercury and oxygen, like this: 2 HgO(s)→2 Hg(1)+O2(g) At a certain temperature, a chemist finds that a 3.3 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the following composition: compound amount HgO 19.5 g Hg 14.6 g O2 0, 17.4 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 x10
Write the equilibrium constant expression. Solid carbon and carbon dioxide gas react and form carbon monoxide: C(s) + CO₂(g) = 2CO(g)
A chemical engineer is studying the following reaction: N₂(g) + 3H₂(g) → 2 NH3(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.018. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel compound pressure expected change in pressure N₂ 11.46 atm ↑ increase ↓decrease (no change) H, 18.35 atm A ↑ increase ↓ decrease (no change) NH3 32.54 atm ↑ increase (no change) N₂ 10.77 atm ↑ increase ↓ decrease ↓decrease ↓decrease decrease B H₂ 16.30 atm (no change) (no change) (no change) ↑ increase 33.91 atm ↑ increase NH3 N₂₂ 11.20 atm ↑ increase ↓ decrease (no change) H₂ 17.58 atm с ↑ increase ↓decrease (no change) NH₂ 33.05 atm ↑…
Consider the following equilibrium for which H = 180.74: N2(g) + O2(g) 2 NO(g) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction?(a) NO(g) is added to the system. (b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%. (d) A catalyst is added to the reaction mixture. (e) The total pressure of the system is increased by adding a noble gas. (f) O2(g) is removed from the system.
A chemical engineer is studying the following reaction: N₂(g) + 3H₂(g) → 2 NH3(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.018. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel compound pressure expected change in pressure N₂ 11.46 atm ↑ increase ↓ decrease (no change) A H₂ 18.35 atm ↑ increase ↓ decrease (no change) NH3 32.54 atm ↑ increase ↓decrease (no change) N2₂ 10.77 atm ↑ increase B H₂ 16.30 atm ↑ increase ↓decrease decrease ↓decrease (no change) (no change) (no change) (no change) NH₂ 33.91 atm O ↑ increase N₂ 11.20 atm ↑ increase C H₂ 17.58 atm O ↑ increase ↓ decrease ↓decrease ↓decrease (no change) NH3…
When nitrogen gas reacts with oxygen gas, nitrogen monoxide gas forms: N2(g) + O2(g) ⇋2NO(g) Initially, 0.40 mol of each reactant is placed into a 2.0 L container and equilibrium is established. If Keq=50.1 for the reaction, what are the equilibrium concentrations of all reactants and products? What two conditions are required, if we want to move reaction forward.