What amount of heat must be supplied to `2xx10^(-2)Kg` of nitrogen at room temperature to rise its temperature by `45^(@)C` at constant pressure? Given molecular mass of nitrogen is 28 and `R=8.3J mol e^(-1)K^(-1)`

Explanation

To solve the problem of calculating the amount of heat required to raise the temperature of nitrogen gas at constant pressure, we can follow these steps:

### Step 1: Identify the given data
- Mass of nitrogen, \( m = 2 \times 10^{-2} \, \text{kg} = 20 \, \text{g} \)
- Change in temperature, \( \Delta T = 45 \, ^\circ C \)
- Molecular mass of nitrogen, \( M = 28 \, \text{g/mol} \)
- Gas constant, \( R = 8.3 \, \text{J/(mol K)} \)

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