A 1.500 L vessel was filled with 0.1600 mol CO and 0.4160 mol H2. When this mixture came to equilibrium at a certain temperature, the vessel contained 0.1010 mol CO. Obtain the value of K. for the following reaction: CO(9) + 2H2 (9) CH,OH(9) K.

A 1.500 L vessel was filled with 0.1600 mol CO and 0.4160 mol H2. When this mixture came to equilibrium at a certain temperature, the vessel contained 0.1010 mol CO. Obtain the value of K. for the following reaction: CO(9) + 2H2 (9) CH,OH(9) K.

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

The equilibrium constant, K., for the following reaction is 1.29×102 at 600 K. COCI,(e)=CO(g) + Cl,(g) Calculate the equilibrium concentrations of reactant and products when 0.270 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K. [COC,] = | M [CO] M [Cl,] M
- Bromine monochloride is synthesized using the reaction Br2(g) + Cl2(g) 2 BrCl(g) Kp = 1.1 x 104 at 150 K A 209.0 L flask initially contains 1.100 kg of Br2 and 1.053 kg of Cl₂. Calculate the mass of BrCl, in in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: What is the percent yield of BrCl? percent yield: grams, that is present g %
The equilibrium constant, K., for the following reaction is 83.3 at 500 K. PCI3(g) + Cl2(9)=PCI5(g) Calculate the equilibrium concentrations of reactant and products when 0.242 moles of PCI3 and 0.242 moles of Cl, are introduced into a 1.00 L vessel at 500 K. [PCI3] =| [Cl2] = [PCI5] = M M
The equilibrium constant, Kc, for the following reaction is 0.0129 at 600 K. COC12 (g) CO(g) + Cl₂ (g) If an equilibrium mixture of the three gases in a 16.3 L container at 600 K contains 0.497 mol of COC1₂(g) and 0.339 mol of CO, the equilibrium concentration of Cl2 is || M.
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI,(g) + Cl, (g) Ke = 1.80 at 250 °C A 0.1978 mol sample of PCl, (g) is injected into an empty 3.15 L reaction vessel held at 250 °C. Calculate the concentrations of PCI, (g) and PCI, (g) at equilibrium. [PCI,] = %3D [PCI,] = M %3D Question Source: MRG - General Chemistry | Pul terms of use | help about us careers privacy policy contact us N prime video P II
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. 1.80 at 250 °C A 0.1952 mol sample of PCl, (g) is injected into an empty 2.15 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCI,] = M [PCI,] = M
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K.PCl3(g) + Cl2(g) PCl5(g)Calculate the equilibrium concentrations of reactant and products when 0.271 moles of PCl3 and 0.271 moles of Cl2 are introduced into a 1.00 L vessel at 500 K.
The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.366 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K
A chemical engineer is studying the following reaction: CH₂CH₂NH₂(aq) + HCl(aq) → Cl¯(aq)+CH₂CH₂NH²(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.82. C The engineer charges ("fills") four reaction vessels with ethylamine and hydrogen chloride, 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.
An equilibrium mixture of PC1, (g), PC1, (g), and Cl₂ (g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl₂ (g) is injected into the mixture, and the total pressure jumps to 263.0 Torr at the moment of mixing. The system then re-equilibrates. The chemical equation for this reaction is PC1₂(g) + Cl₂(g) = PCl, (g) Calculate the new partial pressures, P, after equilibrium is reestablished. PPCL, Pch PPCL, = = = Torr Torr Torr
Consider the following reaction where K. = 1.29x102 at 600 K. COCl»(g) eCO(g) + Cl2(g) A reaction mixture was found to contain 0.107 moles of COCI,(g), 2.44x102 moles of CO(g), and 4.39×102 moles of Cl2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
A chemical engineer is studying the following reaction: 2 NO(g)+2H,(9) - N2(9)+2H,0(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 2.0. The engineer charges ("fills") four reaction vessels with nitrogen monoxide 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 compound pressure expected change in pressure vessel ΝΟ 6.78 atm O f increase Ot decrease O (no change) H, 2.93 atm ↑ increase OI decrease O (no change) A N2 5.23 atm f increase I decrease (no change) H, O 7.24 atm t increase I decrease (no change) NO 5.29 atm f increase I decrease (no change) H, 1.44 atm f increase OI decrease (no change) В N2 5.98 atm increase I decrease (no change) H, O 8.73 atm f increase O I decrease O (no change)…