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CO(g) + 2H2(g) CH₂OH(g) (a) State and explain the effect of using a catalyst on the yield of methanol in this equilibrium. (b) Give an expression for the equilibrium constant (K.) for this reaction. (c) A mixture of carbon monoxide and hydrogen was allowed to reach equilibrium in a container of volume 250 cm³ at temperature T. At equilibrium, the mixture contained 0.340 mol of carbon monoxide, 0.190 mol of hydrogen and 0.0610 mol of methanol. Calculate the value of the equilibrium constant (K.) for this reaction at temperature T. Ke mol-2 dm (d) Methanol decomposes on heating in a reaction that is the reverse of that used in its manufacture. CH OH(g) = CO(g) + 2H2(g) Use your answer from part (c) to determine the value of K. for this equilibrium at temperature T. State the units for this value of K (If you were unable to complete the calculation in part (c), assume a value of K = 0.825 mol-2 dm. This is not the correct value.)

CO(g) + 2H2(g) CH₂OH(g) (a) State and explain the effect of using a catalyst on the yield of methanol in this equilibrium. (b) Give an expression for the equilibrium constant (K.) for this reaction. (c) A mixture of carbon monoxide and hydrogen was allowed to reach equilibrium in a container of volume 250 cm³ at temperature T. At equilibrium, the mixture contained 0.340 mol of carbon monoxide, 0.190 mol of hydrogen and 0.0610 mol of methanol. Calculate the value of the equilibrium constant (K.) for this reaction at temperature T. Ke mol-2 dm (d) Methanol decomposes on heating in a reaction that is the reverse of that used in its manufacture. CH OH(g) = CO(g) + 2H2(g) Use your answer from part (c) to determine the value of K. for this equilibrium at temperature T. State the units for this value of K (If you were unable to complete the calculation in part (c), assume a value of K = 0.825 mol-2 dm. This is not the correct value.)

Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.81P
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Q8. Methanol can be manufactured in a reversible reaction as shown by the equation. Page 12 of 14 CO(g) + 2H₂(g) = CH3OH(g) (a) State and explain the effect of using a catalyst on the yield of methanol in this equilibrium. (b) Give an expression for the equilibrium constant (Kc) for this reaction. (c) A mixture of carbon monoxide and hydrogen was allowed to reach equilibrium in a container of volume 250 cm³ at temperature T. (d) At equilibrium, the mixture contained 0.340 mol of carbon monoxide, 0.190 mol of hydrogen and 0.0610 mol of methanol. Calculate the value of the equilibrium constant (K.) for this reaction at temperature T. K₂ Methanol decomposes on heating in a reaction that is the reverse of that used in its manufacture. CH₂OH(g) CO(g) + 2H₂(g) Use your answer from part (c) to determine the value of K. for this equilibrium at temperature T. State the units for this value of Ke mol-2 dm (If you were unable to complete the calculation in part (c), assume a value of Kc = 0.825 mol-² dm. This is not the correct value.) Page 13 of 14 Value of K Units of K
Transcribed Image Text:Q8. Methanol can be manufactured in a reversible reaction as shown by the equation. Page 12 of 14 CO(g) + 2H₂(g) = CH3OH(g) (a) State and explain the effect of using a catalyst on the yield of methanol in this equilibrium. (b) Give an expression for the equilibrium constant (Kc) for this reaction. (c) A mixture of carbon monoxide and hydrogen was allowed to reach equilibrium in a container of volume 250 cm³ at temperature T. (d) At equilibrium, the mixture contained 0.340 mol of carbon monoxide, 0.190 mol of hydrogen and 0.0610 mol of methanol. Calculate the value of the equilibrium constant (K.) for this reaction at temperature T. K₂ Methanol decomposes on heating in a reaction that is the reverse of that used in its manufacture. CH₂OH(g) CO(g) + 2H₂(g) Use your answer from part (c) to determine the value of K. for this equilibrium at temperature T. State the units for this value of Ke mol-2 dm (If you were unable to complete the calculation in part (c), assume a value of Kc = 0.825 mol-² dm. This is not the correct value.) Page 13 of 14 Value of K Units of K
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