H2 (g) + I, (g)= 2HI (g). When 46 g of I2 and 1.00 g of H2 are heated to equilibrium at 470°C, the equilibrium mixture contains 1.90 g 12. (a) How many moles of each gas are present in the equilibrium mixture? (b) Compute the equilibrium constant. Ans. (a) 0.0075 mol I2, 0.32 mol H2, 0.35 mol HI; (b) K = 50

H2 (g) + I, (g)= 2HI (g). When 46 g of I2 and 1.00 g of H2 are heated to equilibrium at 470°C, the equilibrium mixture contains 1.90 g 12. (a) How many moles of each gas are present in the equilibrium mixture? (b) Compute the equilibrium constant. Ans. (a) 0.0075 mol I2, 0.32 mol H2, 0.35 mol HI; (b) K = 50

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 reaction: 2 NH3(g) = N₂(g) + 3 H₂(g). At T = 740 K, the equilibrium constant K for this reaction is K₂ = 10. 22. What is the correct form of the equilibrium constant K for this reaction? (A) Kc = (B) Kc = (C) Kc = 2[NH3] [N₂] + 3[H₂] (D) Kc = (E) Kc = [N₂][H₂]³ [N₂] + 3[H₂] 2[NH3] [NH3]² [N₂] [H₂] 3³ 3 [N₂] [H₂]³ 2 [NH3]²
The reaction N2O4(g) =* 2NO2(g) has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N2O4 was 0.279 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO2= i atm (b) What was the total pressure of the mixture of gases? total pressure = i atm
3.6
At a certain temperature, 0.391 mol CH, and 0.768 mol H, S are placed in a 3.00 L container. CH,(g) + 2 H,S(g) = CS,(g) + 4 H,(g) At equilibrium, 11.7 g CS, is present. Calculate K.. Ke & TOOLS x10"
The equilibrium constant, Kp, describes the ratio of product and reactant concentrations at equilibrium in terms of partial pressures. Consider the reaction below which has K, of 870 at 25 °C. H;(g) + 1,(g) 2HI(g) (a) Determine the numbers of moles of:- (i) HI formed when H2 = 0.5 moles and I; = 0.5 moles (ii) I2 formed when H2 = 0.5 moles and HI = 1.5 moles
Please answer all (8)
The reaction N204(g) 2NO2(g) has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N204 was 0.127 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO2 = i atm (b) What was the total pressure of the mixture of gases? total pressure = i atm
(a) Formulate the equilibrium expression for the endo- thermic reaction AgCl-NH3(s) = A£CI(s) + NH3(g) (b) What is the effect on PNH, at equilibrium if addi- tional AgCl(s) is added? (c) What is the effect on PNH, at equilibrium if addi- tional NH3(g) is pumped into or out of the system, provided that neither of the two solid phases shown in the chemical equation is completely used up? (d) What is the effect on PNH; of lowering the temperature?
Calculating equilibrium composition from an equilibrium... 0/5 Suppose 500. mL flask is filled with 1.9 mol of H, and o0.50 mol of C1,. The following reaction becomes possible: H, (g) + Cl,(g) – 2HC1(g) The equilibrium constant K for this reaction is 3.61 at the temperature of the flask. Calculate the equilibrium molarity of H,. Round your answer to two decimal places. OM
At a certain temperature, 0.700 mol SO, is placed in a 2.50 L container. 2 SO3 (g) = 2 S0,(g) + 0,(g) At equilibrium, 0.120 mol O, is present. Calculate K.. Ke =
11
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