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What amount of heat must be supplied to `2.0 xx 10^(-2)` kg of nitrogen (at room temperature ) to raise the temperature by `45^(@)C` at constant pressure. Molecular mass of `N_(2) = 28 , R= 8.3 J "mol"^(-1) K^(-1)`.

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To solve the problem of calculating the amount of heat required to raise the temperature of nitrogen gas, we will follow these steps: ### Step 1: Identify the given values - Mass of nitrogen (m) = \(2.0 \times 10^{-2}\) kg - Temperature rise (ΔT) = \(45^\circ C\) - Molecular mass of nitrogen (N₂) = 28 g/mol - Universal gas constant (R) = 8.3 J/(mol·K) ...
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