For a reaction
`CH_(3)OCH_(3)(g) rarr CH_(4)(g)+H_(2)(g) + CO(g)` at `750 K`,
the rate constant is `6.72 xx 10^(-3) min^(-1)`. Starting with a pressure of `400 mm` of `Hg` at this temperature in a closed container, how many minutes would it take for the pressure in the container to become `760 mm Hg` ?

Explanation

To solve the problem, we will follow these steps:

### Step 1: Understand the Reaction and Initial Conditions
The reaction is:
\[ \text{CH}_3\text{OCH}_3(g) \rightarrow \text{CH}_4(g) + \text{H}_2(g) + \text{CO}(g) \]

We start with an initial pressure \( P_0 = 400 \, \text{mm Hg} \) and we want to find out how long it will take for the pressure in the container to reach \( P_t = 760 \, \text{mm Hg} \).

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