If the value of CP for nitrogen gas is 7 JK -1 mol -1, then the value of Δ H on heating 28 g of nitrogen gas from 0° C to 100° C at constant pressure will be

Question

If the value of CP for nitrogen gas is 7 JK -1 mol -1, then the value of Δ H on heating 28 g of nitrogen gas from 0° C to 100° C at constant pressure will be (A) 1200 J (B) 1300 J (C) 1400 J (D) 1500 J

Tardigrade Admin · Accepted Answer

Heat of reaction at constant pressure is given by the equation
Here

Δ H = n C_{p} (T_{2} - T_{1})

C_{p} = 7 J K^{- 1} m o l^{- 1}

weight of

N_{2} g a s = 28 g

T_{1} = 0^{\circ} C = 273 + 0 = 273 K

T_{2} = 10 0^{\circ} C = 273 + 100 = 373 K

Number of moles

= \frac{weight of nitrogen}{molecular weight of nitrogen}

= \frac{28}{14} = 2

Now by using

Δ H = n C_{P} (T_{2} - T_{1})

= 2 \times 7 (373 - 273)

Δ H = 14 \times 100 = 1400 J

Q. If the value of CP​ for nitrogen gas is 7JK−1mol−1, then the value of ΔH on heating 28g of nitrogen gas from 0∘C to 100∘C at constant pressure will be

1200 J

1300 J

1400 J

1500 J

Q. If the value of $C_{P}$ for nitrogen gas is $7 J K^{- 1} m o l^{- 1}$ , then the value of $Δ H$ on heating $28 g$ of nitrogen gas from $0^{\circ} C$ to $10 0^{\circ} C$ at constant pressure will be