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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
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B
650.3kJ
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C
320.5kJ
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D
233.5kJ
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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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