Single Choice

For the reactions, (i) $${H}_{2}(g)+{Cl}_{2}(g)=2HCl(g)+x$$ $$kJ$$ (ii) $$2HCl(g)={H}_{2}(g)+{Cl}_{2}(g)-y$$ $$kJ$$ which one of the following statements is correct?

A$$x-y> 0$$
B$$x-y< 0$$
C$$x-y=0$$
Correct Answer
DNone of these

Solution

Since 1$$^{st}$$ reaction is opposite of the 2$$^{nd}$$ reaction. So, on adding both reactions we will get, $$x - y = 0$$ Hence, answer is option $$C$$.

SIMILAR QUESTIONS

Chemical Thermodynamics

Regarding a thermochemical equation a wrong statement is

Chemical Thermodynamics

Which of the following statements are correct?

Chemical Thermodynamics

$$C(s)\, +\, O_2(g)\, \rightarrow\, CO_2(g);\quad \Delta H\, =\, -\,94.3$$ kcal/mol $$CO(g)\, +\, 1/2\, O_2(g)\, \rightarrow\, CO_2(g);\quad\Delta H\, =\, -\,67.4$$ kcal/mol $$O_2(g)\, \rightarrow\, 2O(g);\quad \Delta H\, =\, 117.4$$ kcal/mol $$CO(g)\, \rightarrow\, C(g)\, +\, O(g);\quad \Delta H\, =\, 230.6$$ kcal/mol Calculate $$\Delta H$$ for $$C (s)$$ $$\rightarrow$$ $$C(g)$$ in Kcal/mol.

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