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Standard XII

Chemistry

Enthalpy of Combustion

When 1.0g o...

Question

When $1.0 g$ of fructose $C_{6} H_{12} O_{6} (s)$ is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter water increases by ${1.56}^{o} C$ . If the heat capacity of the calorimeter and its contents is $10.0 k J /^{o} C$ . Calculate the enthalpy of combustion of fructose at $298 K$

- 2808 k J / m o l

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+ 2808 k J / m o l

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- 280.8 k J / m o l

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None of these

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Solution

The correct option is C $- 2808 k J / m o l$
Heat released by the combustion $= C_{p} \times Δ T = 10 \times 1.56 k J = 15.6 k J$

Hence, $Δ H = - 15.6 k J / g$

Molar mass of fructose $= 180 g$

Hence, $Δ H_{c o m b u s t i o n}$ $= - 15.6 \times 180 k J / m o l = - 2808 k J / m o l$

Hence, option A is correct

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When 1.0g of fructose C6H12O6(s) is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter water increases by 1.56oC. If the heat capacity of the calorimeter and its contents is 10.0 kJ/oC. Calculate the enthalpy of combustion of fructose at 298K

The correct option is C −2808kJ/molHeat released by the combustion =Cp×ΔT=10×1.56 kJ=15.6 kJHence, ΔH=−15.6 kJ/gMolar mass of fructose =180gHence, ΔHcombustion=−15.6×180 kJ/mol=−2808 kJ/molHence, option A is correct