Consider the two gaseous equilibria: SO-(g) +½02(g)= SO;(g) 2S03(g) = SO2(g)+ O2(g) K1 K2 The values of the equilibrium constants K1 and K2 are related by O K2 = K,2 O K22 = K1 O K2 = 1/K1² O K2 = 1/K1 O none of these.

Consider the two gaseous equilibria: SO-(g) +½02(g)= SO;(g) 2S03(g) = SO2(g)+ O2(g) K1 K2 The values of the equilibrium constants K1 and K2 are related by O K2 = K,2 O K22 = K1 O K2 = 1/K1² O K2 = 1/K1 O none of these.

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 following equilibrium reaction: PBr5(g) + 1/2 O2(g) = POB13(g) + Br2(g) Kc = 5.6 x 102 at 512 K Calculate K. for the reaction 2 PBr5(g) + O2(g) = 2 POBR3(g) + 2 Br2(g) at the same temperature. 24 1.1 x 103 280 5.6 x 102 O None of these 3.2 x 105
produces N20 and oxygen. Calculate the value of the equilibrium constant K. for the reaction 2 N,O4(g) –2 N,0(g) + 3 O2(g) from the following information: N2(g) + ¿O2(g) =N‚O(g) K¸ = 2.7 × 10-18 N,O4(g) =2 NO;(g) K. = 4.6 × 10-3 N2(g) + 2 O2(g) =2 NO2(g) K. = 1.7× 10-17
4
For the equilibrium 2lBr(g) = 12(g) + Br2(g) Kc = 8.50 × 10³ at 150 °C. If 0.0600 mol of IBr is placed in a 1.0-L container, what is the partial pressure of I₂(g) in atm after equilibrium is reached?
A gaseous mixture contains 0.27 mol CO, 0.12 mol H2, and 0.022 mol H,O, plus an unknown amount of CH4, in each liter. This mixture is at equilibrium at a certain temperature. CO(9) + 3H, (9) = CH4 (9) + H,O(9) What is the concentration of CH4 in this mixture? The equilibrium constant K, equals 3.99.
At 1100 K, K₂ = 0.30 for the reaction 2SO₂ (g) + O2(g) — 2SO3 (9) What is the value of K at this temperature? K=
At 400 K, an equilibrium mixture of H2, 12, and HI consists of 0.065 mol H2, 0.079 mol 12, and 0.13 mol HI in a 4.50-L flask. What is the value of K, for the following equilibrium? (R= 0.0821 L atm/(K • mol)) 2HI(g) = H2(g) + 12(8) 0.29 8.2 0.039 O 26 3.4
Steam reforming of methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 200. mL flask with 4.2 atm of methane gas and 2.8 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of carbon monoxide gas to be 2.5 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits.
Consider the following reactions: CO (g) + H2O (g) <-> CO2 (g) + H2 (g) | Kp(1)= 0.694 at 1200.K C3H8 (g) + 3 H2O (g) <-> 3 CO (g) + 7 H2 (g) | Kp(2)= 8.175 x 1015 at 1200.K Write the overall equation for the reaction of propane and steam to produce carbon dioxide and hydrogen. Calculate Kp for the overall process at 1200. K. What molecule(s) in the steps are reaction intermediate(s)? If 0.500 atm of CO2, H2, C3H8, and H2O are initially placed in the same container, then given your answer in part a., determine which direction the reaction will shift in order to establish equilibrium.
N2(g) +3H2(g) 2NH3 (g) what is the value of K. at 500 °C if the equilibrium concentrations are as follows: H2 = 0.50 M , N2] = 0.60 M , and [NH3] = 2.2 M ? Express the equilibrium constant to two significant figures. ? Ke =
6. At 27°C, K=2.6 X 105 for the reaction 2 NH3 (g) > N2 (g) + 3 H2 (g) Calculate the value of K for the following: a.) NH3(g) > ½ N2(g) + 3/2 H;(g) b.) N2(g) + 3 H2(g) 2 NH3(g)