Question
1. A team of chemists is studying the following equilibrium, which has the given equilibrium constant...
1. A team of chemists is studying the following equilibrium, which has the given equilibrium constant at a certain temperature:
2 CH4(g) ⇄ C2H2(g) + 3H2(g)
Kp = 2. x 10-7
They fill a reaction vessel at this temperature with 11 atm of methane (CH4) gas. What is the equilibrium pressure of C2H2?
2. Ammonia decomposes to form nitrogen and hydrogen, like this:
2 NH3(g) ⇄ N2(g) + 3 H2(g)
An industrial chemist studying this reaction fills a 25.0 L tank
with 2.2 mol of ammonia gas, and when the mixture has come to
equilibrium measures the amount of hydrogen gas to be 2.3
mol.
Calculate the concentration equilibrium constant
for the decomposition of ammonia at the final temperature of the
mixture.
Round your answer to 2 significant digits in decimal form. (for example: 8.9x102 would be written 890; 8.1x10-2 would be written 0.082)
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