NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Easy

1 of 1

Application +4 | -1

Equal volume of

{C_2}{H_2}

and

{H_2}

are combusted under identical condition. The ratio of their heat of combustion is:

{H_2}(g) + \frac{1}{2}{O_2}(g) \to {H_2}O(g);\Delta H = - 241.8\,\,\,kJ

{C_2}{H_2}(g) + 2\frac{1}{2}{O_2}(g) \to 2C{O_2}(g) + {H_2}O(g);\,\,\Delta H = - 1300\,\,\,kJ

View answer and explanation

Correct option: A

5.37/1

Option A (5.37/1) is correct because the ratio of the heat of combustion is calculated by dividing the heat of combustion of C2H2 by the heat of combustion of H2, considering equal volumes imply equal moles.

More Questions from THERMODYNAMICS

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The internal energy of one mole of a gas is: An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If

{T_i}

is the initial temperature and

{T_f}

is the final temperature, which of the following statements is correct? For which of the process, ∆S is negative? The work done by a weightless piston in causing an expansion ∆V (at constant temperature), when the opposing pressure, P is variable, is given by: Assertion :- At constant pressure of the change

\mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g})

work done is negative.

Reason :- During phase transition work done is always negative. For the reaction,

\mathrm{X}_2 \mathrm{O_4(l}) \longrightarrow 2 \mathrm{XO}_2(\mathrm{g}), \Delta U=2.1 \mathrm{~kcal}, \Delta S=20 \mathrm{~cal} \mathrm{~K}^{-1}

300 \mathrm{~K}

. Hence,

\Delta G