The amount of heat supplied to 4 X $10^{- 2}$ kg of nitrogen at room temperature to rise its temperature by $50 C$ at constant pressure is (Molecular mass of nitrogen is $28$ and $R = 8.3 J$ ${m o l}^{- 1} K^{- 1})$

2.08 k J

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3.08 k J

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4.08 k J

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5.08 k J

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Solution

The correct option is C $2.08 k J$
$E = n C_{p} T$
Finding $C_{p}$ C
$C_{p} - C_{v} = R \Rightarrow 1 - \frac{C_{v}}{C_{p}} = R \Rightarrow 1 - \frac{1}{r} = \frac{R}{C_{p}} \Rightarrow 1 - \frac{5}{7} = \frac{8.3}{C_{p}} \Rightarrow \frac{2}{7} = \frac{8.3}{C_{p}} \Rightarrow C_{p} = 29.05 E = \frac{4}{100 \times 28} \times 29.05 \times 50 K J = 2.075 K J = 2.08 K J$

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The amount of heat supplied to 4 X 10−2 kg of nitrogen at room temperature to rise its temperature by 50C at constant pressure is (Molecular mass of nitrogen is 28 and R=8.3J mol−1K−1)

The correct option is C 2.08kJE=nCpTFinding CpCCp−Cv=R⇒1−CvCp=R⇒1−1r=RCp⇒1−57=8.3Cp⇒27=8.3Cp⇒Cp=29.05E=4100×28×29.05×50KJ=2.075KJ=2.08KJ

The amount of heat supplied to 4 X $10^{- 2}$ kg of nitrogen at room temperature to rise its temperature by $50 C$ at constant pressure is (Molecular mass of nitrogen is $28$ and $R = 8.3 J$ ${m o l}^{- 1} K^{- 1})$