You visited us 1 times! Enjoying our articles? Unlock Full Access!

Calorimetry

A sample of ...

Question

A sample of $0.16 g C H_{4}$ was subjected to the combustion at $27^{o} C$ in a bomb calorimeter. The temperature of the calorimeter. The temperature of the calorimeter system (including water) was found to rise by ${0.5}^{o} C$ . Calculate the heat of combustion of methane at
(i) constant volume and
(ii) constant pressure. the thermal capacity of calorimeter system is $17.0 k J K^{- 1}$ and $R = 8.314 J K^{- 1} m o l^{- 1}$

Open in App

Solution

Amount of heat required = $0.5$ degrees = $17.7$ x $0.5$
= $8.85 K J$
0.16g of methane produces 8.85KJ
Heat liberated by 1 mol of methane = $\frac{8.85}{0.16} \times 16 = 885 K J$
Change in heat =change in energy+nRT
Change of $n = 2$
$Δ H$ = $- 885 + (- 2) (8.3 \times 1 0^{- 3})$
= $- 889.986 K J / M o l$

Suggest Corrections

Similar questions

27^{\circ} C

{0.5}^{\circ} C

x

17.7 k J K^{- 1}

- x

[R = 8.314 J K^{- 1} m o l^{- 1}]

27^{\circ} C

{0.5}^{\circ} C

x

x

17.7 k J K^{- 1}, R = 8.314 J K^{- 1} m o l^{- 1}

27^{\circ}

{0.5}^{\circ}

K^{- 1} .

(R = 8.314 J m o l^{- 1} K^{- 1})]

C H_{4}

27^{o} C

{0.25}^{o} C

Δ H

C H_{4}

27^{o} C

3263.9 k J m o l^{- 1}

25^{o} C

Join BYJU'S Learning Program