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Question

If  $$S + O_2  \rightarrow    SO_2$$     ;     $$\Delta H = - 298.2$$
    $$SO_2 + \frac{1}{2} O_2  \rightarrow  SO_3$$    ;     $$\Delta H = - 98.7$$
    $$SO_3 + H_2O   \rightarrow  H_2SO_4$$       ;      $$\Delta H = - 130.2$$
    $$H_2 + \frac{1}{2} O_2  \rightarrow   H_2O$$    ;    $$\Delta H = - 287.3$$
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
433.5kJ
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Solution

The correct option is A $$-814.4 kJ$$
The thermochemical reactions are as given below.
$$S + O_2  \rightarrow    SO_2,\Delta H = - 298.2$$
$$SO_2 + \frac{1}{2} O_2  \rightarrow  SO_3,\Delta H = - 98.7$$
$$SO_3 + H_2O   \rightarrow  H_2SO_4,\Delta H = - 130.2$$
$$H_2 + \frac{1}{2} O_2  \rightarrow   H_2O,\Delta H = - 287.3$$
The four reactions are added to obtain the reaction $$S +H_2 + 2O_2  \rightarrow  H_2SO_4$$. 
This is the reaction for the formation of $$H_2SO_4$$.
Hence, the enthalpy of formation of $$H_2SO_4$$ is $$-298.2-98.7-130.2-287.3$$
$$=-814.4$$kJ

Chemistry

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