A gas of molecular mass 71 g `mol^(-1)` is enclosed in a vessel at a temperature of `30^@C`. If the pressure exerted by the gas is 1065 mm of Hg, calculate the density of the gas.

Explanation

To calculate the density of the gas, we will use the ideal gas law and the relationship between density, mass, and volume. Here’s a step-by-step solution:

### Step 1: Convert Pressure from mm Hg to atm
The pressure of the gas is given as 1065 mm Hg. We need to convert this to atmospheres (atm) using the conversion factor \(1 \text{ atm} = 760 \text{ mm Hg}\).

\[ P = \frac{1065 \text{ mm Hg}}{760 \text{ mm Hg/atm}} = 1.40 \text{ atm} \]
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