For the reactions: ${\rm{C}} + {{\rm{O}}_2} \to {\rm{C}}{{\rm{O}}_2};\Delta H = - 393{\rm{kJ}}$ $2{\rm{Zn}} + {{\rm{O}}_2} \to 2{\rm{ZnO}};\Delta H = - 412{\rm{kJ}}$ which one is correct?

Oxidation of carbon is not feasible

Oxidation of Zn is not feasible

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Easy

1 of 1

Analyzing +4 | -1

For the reactions:

\mathrm{C} + {\mathrm{O}_2} \to \mathrm{C}{\mathrm{O}_2};\Delta H = - 393\mathrm{kJ}

2\mathrm{Zn} + {\mathrm{O}_2} \to 2\mathrm{ZnO};\Delta H = - 412\mathrm{kJ}

which one is correct?

View answer and explanation

Correct option: A

Carbon can reduce ZnO to Zn

Option D (Zn liberates more heat than carbon during oxidation) is correct because the enthalpy change for the oxidation of Zn is more negative than that of carbon, indicating more heat is released.

More Questions from THERMODYNAMICS

Practice All Chapter MCQs →

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