1. Methane and steam, both with an initial pressure of I atm, are sealed in a 1-litre vessel at 1000K When equilibrium is attained, only 45% of the methane reacted The equation for the reaction is as follows CH. (g) + H2O (g) CO (g) + 3H2 (g) AH=+205 kJ mol a) Calculate the equilibrium constants, K, and K. for the reaction at 1000 K. b) Predict the shift in equilibrium position when the temperature is lowered. c) Explain the effect of lowering the temperature on the Kp value d) Will there be an increase in the yield of H2 (g) if the partial pressure of methane is increased while volume and temperature are kept constant? Justify your answer

1. Methane and steam, both with an initial pressure of I atm, are sealed in a 1-litre vessel at 1000K When equilibrium is attained, only 45% of the methane reacted The equation for the reaction is as follows CH. (g) + H2O (g) CO (g) + 3H2 (g) AH=+205 kJ mol a) Calculate the equilibrium constants, K, and K. for the reaction at 1000 K. b) Predict the shift in equilibrium position when the temperature is lowered. c) Explain the effect of lowering the temperature on the Kp value d) Will there be an increase in the yield of H2 (g) if the partial pressure of methane is increased while volume and temperature are kept constant? Justify your answer

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...

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Consider the following system at equilibrium where K. 7.00x10-5 and AH° = 182 kJ/mol at 673 K. NH4I (s) = NH3 (g) + HI (g) The production of NH3 (g) is favored by: Indicate True (I) or False (F) for each of the following: 1. increasing the temperature. v 2. decreasing the pressure (by changing the volume). v 3. increasing the volume. v 4. adding NH4I . 5. removing HI .
A] HgS occurs in two crystalline forms called "red" and "black". For the conversion of 8. L- the red form to the black form at 525 °C, 4Gº = -0.157 kJ mol-¹ and AH = 4.184 kJ mol-¹. Assuming the AH is temperature independent, find the temperature at which the two forms can coexist at equilibrium at 1.000 bar. Which is more stable above this temperature?
Consider the following system at equilibrium where K. = 9.52x102 and AH° = 18.8 kJ/mol at 350 K. CH4 (g) + CC14 (g) =2 CH,Ch (g) The production of CH,Cl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: |1. decreasing the temperature. | 2. increasing the pressure (by changing the volume). | 3. decreasing the volume. v 4. adding CH,Cl . | 5. removing CCI4 .
For the equilibrium N2(g)+O2 <-->2NO(g), Kp = 0.0017 at 2300 K. At a given point, the partial pressures of the gases are PN2=PO2 = 0.660 atm and PNO= 0.0272atm. Which statment below is true? a. Q < K, so the reaction will continue to make more products. b. Q > K, so the reaction will consume products to make more reactants. c. Q = K, so the system is at equilibrium. d. The value of K will decrease until it is equal to Q. Show your work:
Consider the following equilibrium: 2NH, (g) – N, (g) + 3H, (g) AG° = 34. kJ Now suppose a reaction vessel is filled with 5.02 atm of ammonia (NH,) and 9.40 atm of nitrogen (N,) at 159. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N, tend to rise or fall? fall Is it possible to reverse this tendency adding H2? In other words, if you said the pressure of N, will tend to rise, can that be yes changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of N, will tend to fall, can that be changed to a tendency to rise by adding H2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, needed to reverse it. atm Round your answer to 2 significant digits.
■ W Chapter... G N. O LCG a Ⓒ BA H H The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if K, and Q are within 5% of each other.) (a) 2 NH3(g) = N₂(g) + 3 H₂(g) [NH3] = 0.485 M, [N₂]; = 0.160 M, [H₂] = 0.110 M, K = 18 What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. O To the right, i.e. the product-side. O It will not shift. (b) 2 NH3(9) N₂(g) + 3 H₂(g) What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. P (NH3) = 1.90 atm, P(N₂) = 11.65 atm, P(H₂) = 11.65 atm, K = 6.6x104 O To the right, i.e. the product-side. O It will not shift. (c) 2 SO 3(g) 2 SO₂(g) + O₂(9) What is the reaction quotient? webassign.net [SO3] = 1.65 M, [SO₂), = 1.65 M, [0₂], =…
Consider the following system at equilibrium where AH° = -87.9 kJ, and K. = 83.3, at 500 K. PC13(g) + Cl2(g) =PCI5(g) When 0.31 moles of Cl2(g) are removed from the equilibrium system at constant temperature: The value of K. increase. decrease. remain the same. The value of Qc K.. is greater than is equal to is less than The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium. The concentration of PC13 will increase. decrease. remain the same.
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
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Consider the following system at equilibrium where K. = 34.5 and AH° = -198 kJ/mol at 1150 K. 2 So, (g) + 02 (g) =2 S03 (g) The production of S03 (g) is favored by: Indicate True (T) or False (F) for each of the following: ]1. decreasing the temperature. v 2. increasing the pressure (by changing the volume). | 3. decreasing the volume. 4. removing SO3 . 5. removing O2 -
The reaction mixture below contains 0.112 atm of H2, 0.077 atm of S2, and 0.224 atm of H2S. 2 H2S(g) 2 H2(g) + S2(g) K, = 2.4x104 at a particular temperature. Based on the information provided, select the correct relationship. O Q > K; the reaction will proceed to form more H2S(g). O More experimental data are always needed to answer a question like this. OQ < K; the reaction will proceed to form more products. OQ= K; the reaction is at equilibrium and no change is expected.