ThermochemistryHard
Question
A quantity of 0.3 g of carbon was converted into CO2 producing 2400 cal of heat. When 0.6 g of carbon was converted to CO, 1400 cal of heat were produced. What will be the heat produced when 0.7 g of CO is converted to CO2?
Options
A.1700 cal
B.1633.33 cal
C.700 cal
D.1000 cal
Solution
$C + O_{2} \rightarrow CO_{2};\Delta H = - \frac{2400}{0.3} \times 12 = - 96000\text{ cal}$
$C + \frac{1}{2}O_{2} \rightarrow CO;\Delta H = - \frac{1400}{0.6} \times 12 = - 28000\text{ cal}$
$\text{Now, }CO + \frac{1}{2}O_{2} \rightarrow CO_{2}; $$${ \Delta H = - ( - 96000) - ( - 28000) = - 68000\text{ cal} }{\therefore\text{ Heat produced = }\frac{68000}{28} \times 0.7 = 1700\text{ cal}}$$
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