What amount of heat must be supplied to $2.0 \times 10^{- 2} k g$ of nitrogen (at room temperature) to raise its temperature by $45^{o} C$ at constant pressure? (Molecular mass of $N_{2} = 28 : R = 8.3 m o l^{- 1} K^{- 1}$ .)

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Solution

Mass of nitrogen, $m = 2.0 \times 10^{- 2} k g = 20 g$
Rise in temperature, $Δ T = 45^{o} C$
Molecular mass of $N 2, M = 28$
Universal gas constant, $R = 8.3 J / m o l K$
Number of moles, $n = m / M$
$= (2 \times 10^{- 2} \times 10^{3}$ ) / 28
$= 0.714$
Molar specific heat at constant pressure for nitrogen, Cp = (7/2)R
$= (7 / 2) \times 8.3$
$= 29.05 J m o l^{- 1} K^{- 1}$
The total amount of heat to be supplied is given by the relation:
$Q = n C_{P} Δ T$
$= 0.714 \times 29.05 \times 45$
$= 933.38 J$
Therefore, the amount of heat to be supplied is 933.38 J.

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What amount of heat must be supplied to 2.0×10−2kg of nitrogen (at room temperature) to raise its temperature by 45oC at constant pressure? (Molecular mass of N2=28:R=8.3mol−1K−1.)

What amount of heat must be supplied to $2.0 \times 10^{- 2} k g$ of nitrogen (at room temperature) to raise its temperature by $45^{o} C$ at constant pressure? (Molecular mass of $N_{2} = 28 : R = 8.3 m o l^{- 1} K^{- 1}$ .)