At -7.73 °C the pressure equilibrium constant K, =6.8 × 10° for a certain reaction.Here are some facts about the reaction:• The constant pressure molar heat capacity C,1.76 J·mol-1. K¯!.• If the reaction is run at constant pressure, the volume increases by 14.%.The initial rate of the reaction is 11. mol·L- 1-1•SO Yes.Using these facts, can you calculate K,at 15. °C?O No.If you said yes, then enter your answer at right. Round it to2 significant digits.Yes, and K,will bebigger.If you said no, can you at least decide whether K atYes, and K, will be15. °C will be bigger or smaller than K, at -7.73 °C?smaller.

Answered: Image /qna-images/answer/d45c614d-8239-4b89-b331-3aa362c833df.jpg

At –7.73 °C the pressure equilibrium constant K, =6.8 × 10° for a certain reaction. Here are some facts about the reaction: • The constant pressure molar heat capacity C_ = 1.76 J•mol · K. • If the reaction is run at constant pressure, the volume increases by 14.%. -1 - • The initial rate of the reaction is 11. mol·Ls. O Yes. Using these facts, can you calculate K, at 15. °C?

At –7.73 °C the pressure equilibrium constant K, =6.8 × 10° for a certain reaction. Here are some facts about the reaction: • The constant pressure molar heat capacity C_ = 1.76 J•mol · K. • If the reaction is run at constant pressure, the volume increases by 14.%. -1 - • The initial rate of the reaction is 11. mol·Ls. O Yes. Using these facts, can you calculate K, at 15. °C?

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

Consider the equilibrium system described by the chemical reaction below. Calculate the value of Qc for the initial set reaction conditions in a 2.00 L container: 0.0560 g H2, 4.36 g l2, and 1.32 g HI. H:(g) + lz(g) = 2 HI(g) Based on the given data, set up the expression for Qc and then evaluate it. Do not combine or simplify terms. Qc =
Nitrogen monoxide and water react to form ammonia and oxygen, like this: 4 NO(g)+ 6H,O(g)→ 4 NH3(g)+50,(9) The reaction is endothermic. Suppose a mixture of NO, H,O, NH, and O, has come to equilibrium in a closed reaction vess perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibriL change in composition shift In equilibrium perturbation to the right O to the left The temperature is lowered. The pressure of 02 will O (none) O to the right O to the left ? The temperature is raised. The pressure of NO will O (none)
For the reaction A(g) + 2 B(g) = C(g) the initial partial pressures of gases A, B, and C are all 0.111 atm. Once equilibrium has been established, it is found that Pc = 0.050 atm. What is AG for this reaction (in kJ/mol) at 25°C? kJ/mol
3.) For the following equilibrium reaction2NO2(g) ↔N2O4(g) + Δlook in the Tro text to see what LeChatelier's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. [Hint: remember that PV=nRT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.
Determine the final temperature of a reaction that was initially 25 C, given that its equilibrium constant tripled and the reaction’s enthalpy of formation is 60.15 kJ/mol.
Consider the following equilibrium: N2O4(g) 2NO2 (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 2.78 atm of dinitrogen tetroxide (N204) at 710. °C. Answer the following questions about this system: rise x10 fall Under these conditions, will the pressure of N2O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm X S
For the reaction 2CH,(g) =C,H2(g) + 3H2(g) Ke = 0.155 at 1611 °C. What is K, for the reaction at this temperature? Express your answer numerically. • View Available Hint(s) ? Kp =
Ammonia (NH3) decomposes to form nitrogen gas and hydrogen gas with an enthalpy of 89.4kJ/mol. Aclosed container is charged with 6.0 atm ammonia and heated to 25.0°C. At equilibrium the pressure of H2 is3.60atm. a. Write the balanced reaction.
At -5.92 °C the pressure equilibrium constant K = 5.9 for a certain reaction. P Here are some facts about the reaction: • If the reaction is run at constant pressure, 127. kJ/mol of heat are released. • The constant pressure molar heat capacity C • The net change in moles of gases is -1. = 2.41 J mol -1. K¹. -1 р Yes. ☐ x10 Using these facts, can you calculate K at -27. °C? ○ No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Р If you said no, can you at least decide whether K at -27. °C will be bigger or smaller than K, at −5.92 °C? П Yes, and K, will be р bigger. Yes, and K smaller. will be No. ☑
For the reaction 2 A(g) = B(g) + 3 C(g), we begin with only pure A(g) and the total pressure is 8.00 atm. We attain equilibrium. At equilibrium, the total pressure is 12.00 atm. What is the value of ∆G◦ for this reaction? The temperature is 25.0 ◦C throughout.
8. Consider the equilibrium reaction: N2(g) + O2(g) = 2 NO(g) Kp 4.10 x 10³ at 2000°C a) If 1.00 atm of nitrogen gas and 1.00 atm of oxygen gas is mixed with 0.10 atm of nitrogen monoxide in a 500.0 mL container at 2000°C, in which direction will the reaction proceed to reach equilibrium? Show all work to justify your answer. b) What is the concentration of each gas when equilibrium is reached at 2000°C? Show all your work. Equilibrium Partial Pressures: PN₂ = Po₂ = 1.02 atm and PNO = 0.07 atm Use PV = nRT Answer: Equilibrium Concentrations: [N₂] = [0₂] = 5.47 x 10-3 mol/L and [NO] = 4 x 10+ M
The reaction mixture below contains 0.112 atm of H2, 0.077 atm of S2, and 0.224 atm of H2S. 2 H2S(g) 2 H2(g) + S2(g) K, = 2.4x104 at a particular temperature. Based on the information provided, select the correct relationship. O Q > K; the reaction will proceed to form more H2S(g). O More experimental data are always needed to answer a question like this. OQ < K; the reaction will proceed to form more products. OQ= K; the reaction is at equilibrium and no change is expected.