371545
How much heat energy in joules must be supplied to \(14\;g\) of nitrogen at room temperature to raise its temperature by \(40^\circ C\) at constant pressure? (Mol. wt. of \({N_2} = 28{\rm{ }}g\))
1 \(50\,R\)
2 \(60\,R\)
3 \(70\,R\)
4 \(80\,R\)
Explanation:
As nitrogen is diatomic, its molar specific heat at constant pressure is \(C_{p}=\dfrac{7}{2} R\) No. of moles, \(n=\dfrac{14}{28}=\dfrac{1}{2}\) \(\therefore \Delta Q=n C_{p} \Delta T\) \(=\dfrac{1}{2} \times \dfrac{7}{2} R \times 40=70 R\)
371545
How much heat energy in joules must be supplied to \(14\;g\) of nitrogen at room temperature to raise its temperature by \(40^\circ C\) at constant pressure? (Mol. wt. of \({N_2} = 28{\rm{ }}g\))
1 \(50\,R\)
2 \(60\,R\)
3 \(70\,R\)
4 \(80\,R\)
Explanation:
As nitrogen is diatomic, its molar specific heat at constant pressure is \(C_{p}=\dfrac{7}{2} R\) No. of moles, \(n=\dfrac{14}{28}=\dfrac{1}{2}\) \(\therefore \Delta Q=n C_{p} \Delta T\) \(=\dfrac{1}{2} \times \dfrac{7}{2} R \times 40=70 R\)
371545
How much heat energy in joules must be supplied to \(14\;g\) of nitrogen at room temperature to raise its temperature by \(40^\circ C\) at constant pressure? (Mol. wt. of \({N_2} = 28{\rm{ }}g\))
1 \(50\,R\)
2 \(60\,R\)
3 \(70\,R\)
4 \(80\,R\)
Explanation:
As nitrogen is diatomic, its molar specific heat at constant pressure is \(C_{p}=\dfrac{7}{2} R\) No. of moles, \(n=\dfrac{14}{28}=\dfrac{1}{2}\) \(\therefore \Delta Q=n C_{p} \Delta T\) \(=\dfrac{1}{2} \times \dfrac{7}{2} R \times 40=70 R\)
371545
How much heat energy in joules must be supplied to \(14\;g\) of nitrogen at room temperature to raise its temperature by \(40^\circ C\) at constant pressure? (Mol. wt. of \({N_2} = 28{\rm{ }}g\))
1 \(50\,R\)
2 \(60\,R\)
3 \(70\,R\)
4 \(80\,R\)
Explanation:
As nitrogen is diatomic, its molar specific heat at constant pressure is \(C_{p}=\dfrac{7}{2} R\) No. of moles, \(n=\dfrac{14}{28}=\dfrac{1}{2}\) \(\therefore \Delta Q=n C_{p} \Delta T\) \(=\dfrac{1}{2} \times \dfrac{7}{2} R \times 40=70 R\)