Methanol, CH, OH, formerly known as wood alcohol, is manufactured commercially by the following reaction: CO(g) + 2H₂(g) → CH₂OH(g) A 1.500 L vessel was filled with 0.1470 mol CO and 0.3900 mol H₂. When this mixture came to equilibrium at 500 K, the vessel contained 0.1340 mol CO. How many moles of each substance were in the vessel at equilibrium? mol CO mol H₂ mol CH,OH

Methanol, CH, OH, formerly known as wood alcohol, is manufactured commercially by the following reaction: CO(g) + 2H₂(g) → CH₂OH(g) A 1.500 L vessel was filled with 0.1470 mol CO and 0.3900 mol H₂. When this mixture came to equilibrium at 500 K, the vessel contained 0.1340 mol CO. How many moles of each substance were in the vessel at equilibrium? mol CO mol H₂ mol CH,OH

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, 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.
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) PC13(g) + Cl₂(g) K = 1.80 at 250 °C A 0.4044 mol sample of PCI, (g) is injected into an empty 4.40 L reaction vessel held at 250 °C. Calculate the concentrations of PCI, (g) and PCI, (g) at equilibrium.
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.
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K.H2 (g) + I2 (g) 2 HI (g)Calculate the equilibrium concentrations of reactants and product when 0.228 moles of H2 and 0.228 moles of I2 are introduced into a 1.00 L vessel at 698 K. [ H2 ] = M [ I2 ] = M [ HI ] = M
Consider the following reaction at a certain temperature: 4 Fe(s) + 3 O2(g)→ 2 Fe203(s) An equilibrium mixture contains 1.2 mol Fe, 0.00090 mol O2, and 2.0 mol Fez03 all in a 2.0-L container. Calculate the value of K for this reaction. K =
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K.H2 (g) + I2 (g) 2 HI (g)Calculate the equilibrium concentrations of reactants and product when 0.334 moles of H2 and 0.334 moles of I2 are introduced into a 1.00 L vessel at 698 K. [ H2 ] = M [ I2 ] = M [ HI ] = M
The equilibrium constant, K., for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g) = 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.351 moles of H, and 0.351 moles of I, are introduced into a 1.00 L vessel at 698 K. [H2 ] = M [I ] M [HI ] = M
Carbon tetrachloride can be produced by the following reaction: C5₂(g) + 3Cl₂(g) + S₂Cl₂(g) + CCl₂) In an experiment, 0.120 mol of CS₂ and 0.360 mol of Cly were placed in a 1.00-L flask at a particular temperature. After equilibrium has been achieved, the mixture contains 0.040 mol CCl Calculate the value of K under the experimental conditions
20.
A student ran the following reaction in the laboratory at 588 K: CO(g) + Cl₂(g) —COCI₂(g) When she introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 1.74 atm and the initial partial pressure of Cl2 was 0.951 atm, she found that the equilibrium partial pressure of COCI₂ was 0.685 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр =
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. = 1.80 at 250 °C A 0.3668 mol sample of PCI, (g) is injected into an empty 4.30 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCI, (g) at equilibrium. [PCl,] = M [PCI,] = M