Question 4 Consider the gas phase equilbrium, N2 +3 H2 --2 N+3. For this reaction, AGo - 50 kJ at 400 °c What is the value of the equilibrium constant. K, at 400 9C? (Note G ive value in non sclenitilic notation, use decimals) Tuesday October 17 2017 7 49 50 PM CDT
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Related questions
Consider the reaction,
N2(g) + 3H2(g) â 2NH3(g);
Suppose that initially 1 mole of N2 and 3 mole of H2 are introduced into a reaction vessel held at T = 673 K and P = 1 bar where the equilibrium constant is K=1.6 Ã10-4. You may assume the vessel resembles a piston with a constant applied pressure of 1 bar.
b) Next, fill in the reaction progress chart on the next page where ε is the number of moles of N2 consumed. Assume ideal gas behavior and use,
dG /dε=âGr° + RT lnQ with Q
Reaction extent, x | Pressure N2 (bars) | Pressure H2 (bars) | Pressure NH3 (bars) | Reaction Quotient, Q | dG / de (kJ/mole) |
e | (1- e)/(4-2 e) | (3- 3e)/(4-2 e) | 2 e/(4-2 e) | ||
0 | 0.25 | 0.75 | 0 | 0 | - ¥ |
0.001 | 0.2499 | 0.7496 | 5.003 e-4 | 2.378 e-6 | -23.52 |
0.002 | |||||
0.003 | |||||
0.004 | |||||
0.005 | |||||
0.006 | |||||
0.007 | |||||
0.008 | |||||
0.009 | |||||
0.01 | 0.2487 | 0.7462 | .005025 | 2.443 e-4 | 2.385 |
* Note that the pressure columns above were calculated using the mole fraction times the total pressure (which is set to 1bar). Hence, for N2 the mole fraction is (1-ε)/(4-2ε), where the total number of moles is 1-ε + 3-3ε+2ε = 4-2ε.