Question

# If $$S + O_2\longrightarrow SO_2;\,\Delta H = -298.2\,kJ$$$$SO_2 + 1/2O_2\longrightarrow SO_3;\,\Delta H = -98.7\,kJ$$$$SO_3 + H_2O\longrightarrow H_2SO_4;\,\Delta H = -130.2\,kJ$$$$H_2 + 1/2O_2\longrightarrow H_2O; \Delta H = -287.3\,kJ$$Then the enthalpy of formation of $$H_2SO_4\,at\,298\,K$$ is :

A
814.4kJ
B
650.3kJ
C
320.5kJ
D
233.5kJ

Solution

## The correct option is A $$-814.4\,kJ$$According to Hess law,enthalpy of formation of $$H_2SO_4\,at\,298\,K$$ is sum of all $$S + O_2\longrightarrow SO_2;\,\Delta H = -298.2\,kJ$$$$SO_2 + 1/2O_2\longrightarrow SO_3;\,\Delta H = -98.7\,kJ$$$$SO_3 + H_2O\longrightarrow H_2SO_4;\,\Delta H = -130.2\,kJ$$$$H_2 + 1/2O_2\longrightarrow H_2O; \Delta H = -287.3\,kJ$$$$\Delta H$$ =$$-298.2\,-98.7 - 130.2 - 287.3 =$$ $$-814.4\,kJ$$Chemistry

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