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Base your answers to questions 69 through 72 on the information below and on your knowledge of chemistry.

Millions of tons of ammonia are produced each year for use as fertilizer to increase food production. Most of the hydrogen needed to produce ammonia comes from methane gas reacting with steam. This reaction, which occurs in a container under controlled conditions, is shown below in unbalanced equation 1.

Equation 1: CH₄(g) + H₂O(g) energy → CO(g) + H₂(g)

The reaction that produces ammonia is represented by balanced equation 2, shown below. A catalyst can be used to increase the rate of the reaction.

Equation 2: N₂(g) + 3H₂(g) → 2NH₃(g) + energy

 A potential energy diagram for equation 2 is shown below.

69 Balance equation 1 in your answer booklet, using the smallest whole-number coefficients. [1]

__ CH₄(g)+  __H₂O(g) +  energy → __ CO(g) + __ H₂(g)

70 Explain, in terms of collision theory, why an increase in temperature increases the rate of reaction between methane gas and steam. [1]

71 State what is represented by interval A on the potential energy diagram. [1]

72 Determine the number of moles of hydrogen gas required to react completely with 50.0 moles of nitrogen gas in the production of ammonia. [1]