Reference no: EM13684720
Question 1:
A mixture of water and graphite is heated to 890 K in a 10 L container. When the system comes to equilibrium it contains 0.875 mol each of CO and H2 and 0.289 mol of H2O and some graphite. Some O2 is added to the system and a spark is applied so that the H2 reacts completely with the O2 forming H2O. Find the amount of CO in the flask when the system returns to equilibrium.
Question 2:
Consider the reaction:
2 H2S (g) + SO2 (g) ↔ 3S (s) + 2 H2O (g)
A reaction mixture initially containing 0.600 bar each of H2S and SO2 was found to contain 0.0054 bar of H2O at equilibrium at 1300 K. A second reaction mixture at the same temperature initially contains 0.500 bar of H2S and 0.350 bar of SO2. Calculate the equilibrium concentrations of all reactants and products at equilibrium.
Question 3:
Hydrogen can be extracted from natural gas according to the reaction:
CH4(g) + CO2(g) ↔ 2 CO (g) + 2 H2 (g) K = 4.5 x 102 at 1115 K
An 85.0 L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 1115 K. Assuming ideal gas behaviour, calculate the mass of H2 (in g) present in the reaction mixture at equilibrium. What is the percent yield of the reaction under these conditions?
Question 4:
The equilibrium constant for the reaction SO2 (g) + NO2 (g) ↔ SO3 (g) + NO (g) is 15.6 at 1000 K. Find the amount of NO2 that must be added to 2.4 mol of SO2 in order to form 1.2 mol of SO3 at equilibrium.
Question 5:
Solid carbon can react with gaseous water to form carbon monoxide gas and hydrogen gas. The equilibrium constant for the reaction at 700 K is Kp = 1.60 x 10-3. If a 1.55 L reaction vessel initial contains 145 mbar of water at 700.0 K in contact with excess solid carbon, find the percent by mass of hydrogen gas of the gaseous reaction mixture at equilibrium.
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