Question

Large quantities of hydrogen gas can be produced industrially by the steam reformation of natural gas. The equation for this reaction is shown below. \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{~g}) \Delta

\mathrm{H}=+206 \mathrm{~kJ} \mathrm{~mol}^{-1} For this reaction, which of the following changes will decrease the amount of H2(g) for a system initially at equilibrium? I. decreasing temperature II. increasing the volume III. adding a catalyst А.I only В.II only С.I and II only D.I, II and III

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