4. Consider the following reaction: CO(g) + 2H₂(g) = CH₂OH(g) An equilibrium mixture for this reaction at a certain temperature was found to have [CO] = 0.105 M, [H₂] = 0.114 M, and [CH3OH] = 0.185 M. What is the value of the equilibrium constant (Kc) at this temperature?

4. Consider the following reaction: CO(g) + 2H₂(g) = CH₂OH(g) An equilibrium mixture for this reaction at a certain temperature was found to have [CO] = 0.105 M, [H₂] = 0.114 M, and [CH3OH] = 0.185 M. What is the value of the equilibrium constant (Kc) at this temperature?

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

A student ran the following reaction in the laboratory at 538 K:COCl2(g) CO(g) + Cl2(g)When she introduced 1.24 moles of COCl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 3.76×10-2 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.Kc =
For the reaction 2NO(g) + O2(g) → 2NO2(g) at a certain temperature, the equilibrium concentrations were found to be [NO2] = 5.7 × 10–3 M, [O2]= 1.0 × 10–2 M, and [NO] = 2.0 × 10–3 M. Calculate the value of the equilibrium constant from these data.
Consider the following equilibrium reaction:H2(g) + I2(g) ↔ 2HI(g)If the following equilibrium concentrations are observed: [H2] = 4.10 x 10-1M, [I2] = 5.54 x 10-2M, [HI] = 3.50 x 10-2M; what is the equilibrium constant
A student ran the following reaction in the laboratory at 682 K:2HI(g) H2(g) + I2(g)When she introduced HI(g) at a pressure of 5.24 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of HI(g) to be 4.15 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction.Kp =
A student ran the following reaction in the laboratory at 697 K:2HI(g) H2(g) + I2(g)When he introduced HI(g) at a pressure of 4.46 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of HI(g) to be 3.52 atm.Calculate the equilibrium constant, Kp, he obtained for this reaction.Kp =
An equilibrium reaction has a K = 3.2 x 10-4. What can be said about the reaction? [Reactants] [Products] [Reactants]> [Products] [Reactants] [Products] < =
3. Nitrogen gas and oxygen gas can combine to produce nitrogen monoxide. At 1500 K the equilibrium constant, Ke, is 1.0 x 10 . Suppose a sample of air has [N2] = 0.80 M and [O2] = 0.20 M before any reaction occurs. Calculate the equilibrium concentrations of product and reactants at equilibrium at this temperature.
The following reaction has an equilibrium constant, Kc equal to 3.59 at 900 °C. CH4(g) + 2H₂S(g) — CS2(g) + 4 H2(g) At a particular time during the reaction, the following composition has been found: [CH4(g)] = 1.20 M, [CS2(g)] = 1.15 M, [H₂S(g)] = 1.31 M, [H2(g)] = 1.85. Predict the activity of the reaction during the particular time above. The reaction should go to the left (or reverse) The reaction should go to the right (or forward) The reaction is at a standstill The reaction activity cannot be determined There is no basis for prediction.
At 773 °C, a mixture of CO(g), H2(g), and CH3OH(g) was allowed to come to equilibrium. The concentrations were determined to be: [CO] = 0.105 M, [H2] = 0.250 M, [CH3OH] = 0.00261 M. Calculate K. for the reaction CO(g) + 2H2(g) CH3OH(g) Kc = %3D
A student ran the following reaction in the laboratory at 282 K: 2CH2C12(g)=CH4(g)+ CCI4(g) When she introduced 6.98x102 moles of CH,Ch(g) into a 1.00 liter container, she found the equilibrium concentration of CH,Cl2(g) to be 4.62x10³ M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =
In an analysis of the following reaction at a certain temperature, Br2(g) + Cl½(g) = 2BrCl(g) the equilibrium concentrations were found to be [Br2] = 4.0 × 10 M, [Cl,] = 2.6 × 10¯² M, and [BrCl] = 2.1 × 10 ² M. Write the equilibrium expression, and calculate the equilibrium constant for this reaction at this temperature. %3D K. = K=