JEE CHEMISTRY MCQ: THERMODYNAMICS

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Application +4 | -1

2.56 \mathrm{~g}

of sulphur is burnt in a constant volume calorimeter with excess of

\mathrm{O}_2(g)

. Temperature increases from

21.25^{\circ} \mathrm{C}

26.72^{\circ} \mathrm{C}

. The bomb has a heat capacity of

923 \mathrm{~J} \mathrm{~K}^{-1}

. Calorimeter contains

815 \mathrm{~g}

of water. Thus, change in internal energy per mole of

\mathrm{SO}_2

formed for the reaction is

\mathrm{S}_8(s)+8 \mathrm{O}_2(g) \longrightarrow 8 \mathrm{SO}_2(g)

(Specific heat of water is

4.184 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~g}^{-1}

)

View answer and explanation

Correct option: A

-296.27 \mathrm{~kJ}

Option A (-296.27 kJ) is correct because the change in internal energy per mole of SO2 formed is calculated using the heat capacity of the calorimeter and the specific heat of water.

More Questions from THERMODYNAMICS

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Consider following reactions
I:

\ \mathrm{C}(\mathrm{s})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})-\mathrm{CO}(\mathrm{g}), \Delta \mathrm{H}_1=\mathrm{a}

II:

\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})-\mathrm{CO}_2(\mathrm{~g}), \Delta \mathrm{H}_2=\mathrm{b}

III:

\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})-2 \mathrm{CO}(\mathrm{g}) ; \Delta \mathrm{H}_3=\mathrm{c}

Select the correct statement When

0.18 \mathrm{~g}

of glucose was burnt in a bomb calorimeter, the temperature rose by

4 \mathrm{~K}.

The heat capacity of the calorimeter system is

\left(\Delta_{\mathrm{C}} \text{H}^{\circ}=-2.8\times 10^6 \mathrm{~J} / \mathrm{mol} \text{ glucose}\right)

Statement-1:

{CsI}

is less soluble in water compared to

{CsCl}

Satement-2: More amount of heat is liberated during the formation of

{CsCl}

than the formation

{Cs} I

from their elements Consider the following processes :

\begin{array}{cccccccccccccccccccc} {}&{\Delta H(KJ/mol)} \\ {1/2A \to B}&{ + 150} \\ {3B \to 2C + D}&{ - 125} \\ {E + A \to 2D}&{ + 350} \end{array}

For

{B}+{D} \rightarrow {E}+2 {C}, \Delta {H}

will be : The difference b/w

\Delta H

and

\Delta u

at constant volume is equal to The heat evolved in the combustion of methane is given by the following equations

\mathrm{C}{\mathrm{H}_4}\left( \mathrm{g} \right) + 2{\mathrm{O}_2}\left( \mathrm{g} \right) \to \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right) + {\mathrm{H}_2}\mathrm{O}\left( l \right);\Delta H = - 890.3\mathrm{kJ}

How many grams of methane would be required to produce 44.15 kJ of heat of combustion?