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: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 5ALQ

See similar textbooks

Similar questions

If wet silver carbonate is dried in a stream of hot air. the air must have a certain concentration level of carbon dioxide to prevent silver carbonate from decomposing by the reaction Ag2CO3(s)Ag2O(s)+CO2(g) H for this reaction is 79.14 kJ/mol in the temperature range of 25 to 125C. Given that the partial pressure of carbon dioxide in equilibrium with pure solid silver carbonate is 6.23 103 torr at 25C, calculate the partial pressure of CO2 necessary to prevent decomposition ofAg2CO3 at 110C. (Hint: Manipulate the equation in Exercise 79.)
For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at this temperature in units of kJ/mol.
Methanol can be synthesized by means of the equilibriumreaction CO(g)+2H2(g)CH3OH(g) for which the equilibrium constant at 225°C is 6.08103. Assume that the ratio of the pressures of CO(g) and H2(g) is 1:2. What values should they have if the partial pressureof methanol is to be 0.500 atm?
Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7 J/mol K. Calculate the equilibrium partial pressures of I2(g), H2(g), and HI(g) for the system 2HI(g)H2(g)+I2(g) at 500°C if the initial partial pressures are all 0.200 atm.
For the given chemical equilibrium, these data are determined experimentally: T K 350K 3.76102 450K 1.86101 Determine H for this reaction.
Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.
100 mmol of (NH3), 300 mmol, are introduced into a 2 L container at 127 °C of (H2) and 200 mmol of (N2). A thermometer and a pressure gauge connected to the container show that the reaction between Nitrogen and Hydrogen occurs at 127 ° C and that said reaction reaches equilibrium marking a pressure of 7.1 bar. Find the equilibrium constant Kp °, considering that ?G ° 400K = −11.92 kj/mol Find the amount of substance (in mmol) that will be had for each species when the reaction has reached equilibrium.
When the reaction FeO (s) + CO (g) ↔ Fe (s) + CO2 (g) takes place at 600 K, it is observed that XCO = 0.526 and XCO2 = 0.474If Kp values are 4.885 and 0.396 at 300 and 1000 K, respectively, calculate ∆H0, ∆G0 and ∆S0 at 600 K. Use all the data available. Result: -8853 J/mol, 520 J/mol, -1562 J/mol K
When the reaction FeO (s) + CO (g) ↔ Fe (s) + CO2 (g) takes place at 600 K, , it is observed thata) Calculate Kp at that temperature. b) If Kp values are 4.885 and 0.396 at 300 and 1000 K, respectively, calculate ∆H0, ∆G0 and ∆S0 at 600 K. Use all the data available.
The following reaction is carried out at 1 atm pressure.CH3COOH (l) + C2H5OH (l) → CH3COOC2H5 (l) + H2O (l)What is the equilibrium constant for this reaction at 200 ºC? What is thecomposition of the mixture if initially 2 mol acetic acid and 2 mol of ethanol werepresent?Note: take the required data from the Perry hand book or any other propertytables
(a) For the ideal gas reaction A + B ↔ 2C + 2D, it is given that ∆Gθ500= 1250 cal mol-1. If 1.0 mol of A and 1.0 mol of B are placed in a vessel at 500 K and P is held fixed at 1200 torr, calculate the equilibrium amount of A, B, C, and D.