Question:
How much heat energy in joule must be supplied to \(14\) g of nitrogen at room temperature to raise its temperature by \(40^{\circ }\)C at constant pressure?
(molecular wt. of nitrogen = \(28\) g, \(R\) = gas constant) (gas is diatomic)
How much heat energy in joule must be supplied to \(14\) g of nitrogen at room temperature to raise its temperature by \(40^{\circ }\)C at constant pressure?
(molecular wt. of nitrogen = \(28\) g, \(R\) = gas constant) (gas is diatomic)
(molecular wt. of nitrogen = \(28\) g, \(R\) = gas constant) (gas is diatomic)
Show Hint
Find the number of moles, use Cp equal to seven halves R for a diatomic gas, and multiply by the temperature rise.
Updated On: Nov 12, 2026
- \(50R\)
- \(60R\)
- \(70R\)
- \(80R\)
Show Solution
Verified By Collegedunia
The Correct Option is C
Solution and Explanation
Step 1: Understanding the Concept
At constant pressure, \(Q=nC_{P}\Delta T\). For a diatomic gas, \(C_{P}=\frac{7}{2}R\).
Step 2: Number of Moles
\(n=\frac{14}{28}=0.5\).
Step 3: Calculation
\(Q=0.5\times\frac{7}{2}R\times40\)
\(Q=70R\).
Final Answer:
The heat required is 70R joules. \[ \boxed{\text{(C) }70R} \]
At constant pressure, \(Q=nC_{P}\Delta T\). For a diatomic gas, \(C_{P}=\frac{7}{2}R\).
Step 2: Number of Moles
\(n=\frac{14}{28}=0.5\).
Step 3: Calculation
\(Q=0.5\times\frac{7}{2}R\times40\)
\(Q=70R\).
Final Answer:
The heat required is 70R joules. \[ \boxed{\text{(C) }70R} \]
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