5 moles of unknown gas is heated at constant volume from to . The molar specific heat of this gas at constant pressure

Question

5 moles of unknown gas is heated at constant volume from $10 ° C$ to $20 ° C$ . The molar specific heat of this gas at constant pressure $C_{p} = 8 cal/mol·°C$ and $R = 8.36 J/mol·°C$ . The change in the internal energy of the gas is __________ calorie. [2026]

Smart Achievers · Accepted Answer

(300)

$C_{p} - C_{v} = R \Rightarrow C_{v} = (C_{p} - R)$

$C_{v} = 6 cal/mol \cdot {}^{\circ}C$

$Δ U = n C_{v} Δ T = 5 \times 6 \times 10 = 300 cal$

Solution

Q.
5 moles of unknown gas is heated at constant volume from $10 ° C$ to $20 ° C$ . The molar specific heat of this gas at constant pressure $C_{p} = 8 cal/mol·°C$ and $R = 8.36 J/mol·°C$ . The change in the internal energy of the gas is __________ calorie. [2026]

Ans.
(300)

$C_{p} - C_{v} = R \Rightarrow C_{v} = (C_{p} - R)$

$C_{v} = 6 cal/mol \cdot {}^{\circ}C$

$Δ U = n C_{v} Δ T = 5 \times 6 \times 10 = 300 cal$

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Solution

Q. 5 moles of unknown gas is heated at constant volume from 10°C to 20°C. The molar specific heat of this gas at constant pressure Cp=8 cal/mol·°C and R=8.36 J/mol·°C. The change in the internal energy of the gas is __________ calorie. [2026]

Ans. (300) Cp-Cv=R⇒Cv=(Cp-R) Cv=6 cal/mol·C∘ ΔU=nCvΔT=5×6×10=300 cal

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Q.
5 moles of unknown gas is heated at constant volume from $10 ° C$ to $20 ° C$ . The molar specific heat of this gas at constant pressure $C_{p} = 8 cal/mol·°C$ and $R = 8.36 J/mol·°C$ . The change in the internal energy of the gas is __________ calorie. [2026]

Ans.
(300)

$C_{p} - C_{v} = R \Rightarrow C_{v} = (C_{p} - R)$

$C_{v} = 6 cal/mol \cdot {}^{\circ}C$

$Δ U = n C_{v} Δ T = 5 \times 6 \times 10 = 300 cal$