Metal oxides can be reduced with hydrogen gas to give the metal. H2(g) + ZnO(s) H2O(g) + Zn(s) Predict the effect of each of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) Add more ZnO(s). (b) Add more H2(g). (c) Remove some Zn(s).
Metal oxides can be reduced with hydrogen gas to give the metal.
H2(g) + ZnO(s) H2O(g) + Zn(s)
Predict the effect of each of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made.
(a) Add more ZnO(s).
(b) Add more H2(g).
(c) Remove some Zn(s).
(d) Remove some water vapor.
(e) In which direction does the equilibrium shift when you raise the temperature?
(f) Calculate the value of ∆Go for the reaction. (You may look up values in tables).
(g) Is the reaction predicted to be spontaneous under standard conditions at 25 degrees Celsius?
(h) Is the equilibrium constant for the reaction greater than 1 or less than 1?
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