14.20 A reaction vessel contains NH3, N2, and H, at equi- librium at a certain temperature. The equilibrium concentrations are [NH3] = 0.25 M, [N2] = 0.11 M, and [H2] = 1.91 M. Calculate the equilibrium con- stant K. for the synthesis of ammonia if the reaction is represented as (a) N2(8) + 3H2(g) = 2NH3(8) (b) N2(8) + H2(g) = NH3(8)

14.20 A reaction vessel contains NH3, N2, and H, at equi- librium at a certain temperature. The equilibrium concentrations are [NH3] = 0.25 M, [N2] = 0.11 M, and [H2] = 1.91 M. Calculate the equilibrium con- stant K. for the synthesis of ammonia if the reaction is represented as (a) N2(8) + 3H2(g) = 2NH3(8) (b) N2(8) + H2(g) = NH3(8)

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

At 500K, the methanol decomposes according to the following reaction, CH3ОН(9) — COog) + 2 H2(g) K= 9.60×10-2 Some methanol, CH3OH (molar mass: 32 g/mol), is placed into a rigid 2.00-L vessel, and the temperature is raised to 500K. If the concentration of CO in the equilibrium mixture is 0.246M, what is the initial concentration of methanol? O A. 0.620 M О в. 1.109 м O. 0.231 M O D. 0.135 M O E. 0.866 M
The equilibrium constant, Kp, for the following reaction is 2.20x10 at 723K. 2NH3(g) N3(g)+3H3(g) If an equilibrium mixture of the three gases in a 11.3 L container at 723K contains NH at a pressure of 1.27 atm and N, at a pressure of 0.599 atm, the equilibrium partial pressure of H, is atm.
A chemical engineer is studying the following reaction: N2(9)+3H,(g) → 2NH,(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.00029. The engineer charges ("fills") three reaction vessels with nitrogen and hydrogen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction compound pressure expected change in pressure vessel N2 52.94 atm f increase OI decrease (no change) H2 23.44 atm O t increase OI decrease O (no change) A NH3 14.08 atm O t increase I decrease (no change) N2 47.16 atm O f increase I decrease (no change) В H2 20.07 atm O f increase O I decrease (no change) NH3 11.95 atm O f increase OI decrease (no change) N2 47.80 atm O f increase OI decrease (no change) H2 21.97 atm O f increase OI decrease (no…
A sample of HI was placed in a container and the following reaction was allowed to come equilibrium. H₂(g) + 1₂(g) = 2 HI(g) The equilibrium concentrations were found to be [HI] = 3.88 M and [H₂] = [1₂] = 0.556. Calculate the equilibrium const Kc, for the reaction. Note Kc is often called K.
A sample of IBr decomposes according to the following equation: 2 IBr(g) 1 I2(g) + 1 Br2(g) An equilibrium mixture in a 1-L vessel at 1926 oC, contains 0.00946 g of IBr, 0.0122 g of I2, and 0.00475 g of Br2.(a) Calculate KP for this reaction at this temperature.KP = (b) What is the total pressure exerted by the equilibrium mixture of gases?Ptotal = atm.
The equilibrium constant (Kc ) for the reaction: PCl3 + Cl2 <=> PCl5 equals 51 at 235°C. If 0.648 mol of phosphorus trichloride and 0.748 mol chlorine (Cl2) are added to a 9.00 L reaction vessel, what is the amount of moles of Cl2 at equilibrium in the mixture at 235°C?
At 500K, the methanol decomposes according to the following reaction, CH3OH(g) = CO(g) + 2 H2(g) K= 9.60×10-2 Some methanol, CH3OH (molar mass: 32 g/mol), is placed into a rigid 2.00-L vessel, and the temperature is raised to 500K. If the concentration of H2 in the equilibrium mixture is 0.246M, what is the initial concentration of methanol? O A, 0.231 M Ов. 0.866 М OC 0.200 M OD. 1.109 M O E. 0.012 M
Consider the reaction, 2AB2(g) = A2(g) + 2B2(g), Kc = 0.263 at 25°C. The reaction begins with an unknown concentration of AB2 in the reaction flask. At equilibrium, the concentration of AB2 is found to be 0.00545 M. a) Complete the ICEE table below, b) Write the equilibrium expression and equation for this reaction (pay close attention to coefficients!), c) Calculate the equilibrium concentration of both products, and d) Calculate the initial concentration of AB2. You should confirm that your equilibrium concentrations will give the correct equilibrium constant when plugged into the expression. ICEE table I C E 2 AB₂(g) A₂(g) + 2 B₂(g)
1. 2.00 moles of ammonia are heated in a sealed 1.00 L container at 650°C. At this temperature, ammonia decomposes to nitrogen and hydrogen gas. 2 NH3 (g) = N2 (g) + 3 H2 (g) At equilibrium, the concentration of ammonia in the container is 1.00 M. What is the value of Ke for this reaction at 650°C?
2) For the reaction, PCI:(g) = PCl:(g) + Ch(g) at 327°C, the equilibrium constant, Ke is 0.234. Suppose that 2.082 g PCIIS is placed in an evacuated 200 mL bulb, which is then heated to 327°C. (R = 0.082 L atm mol'K', PCIS = 208.2 g/mol) (a) What would be the pressure of PCIs if it did not dissociate? (b) What is the partial pressure of PCIS at equilibrium? (c) What is the total pressure in the bulb at equilibrium? (d) What is the fraction of PCIS at cquilibrium?
The reaction N204(s) * 2NO2(3) 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 0.183 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of N02 = atm (b) What was the total pressure of the mixture of gases? total pressure = atm