A) 1200 J
B) 1300 J
C) 1400 J
D) 1500 J
Correct Answer: C
Solution :
Key Idea Heat of reaction at constant pressure is given by the equation \[\Delta H=n{{C}_{p}}({{T}_{2}}-{{T}_{1}})\] Here \[{{C}_{p}}=7\,J{{K}^{-1}}\,mo{{l}^{-1}}\] weight of \[{{N}_{2}}\] gas = 28 g \[{{T}_{1}}={{0}^{o}}C=273+0=273\,K\] \[{{T}_{2}}={{100}^{o}}C=273+100=373\,K\] Number of moles \[=\frac{weight\text{ }of\text{ }nitrogen}{molecular\text{ }weight\text{ }of\text{ }nitrogen}\] \[=\frac{28}{14}=2\] Now by using \[\Delta H=n\,{{C}_{p}}({{T}_{2}}-{{T}_{1}})\] \[=2\times 7\,(373-273)\] \[\Delta H=14\times 100=1400\,J\]
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