JEE CHEMISTRY MCQ: THERMODYNAMICS

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Application +4 | -1

The carbon dioxide exhaled in the breath of astronaut is often removed from the spacecrafts by reaction with lithium hydroxide.

2 \mathrm{LiOH}(\mathrm{s})+\mathrm{CO}_2(\mathrm{g}) \rightarrow \mathrm{Li}_2 \mathrm{CO}_3(\mathrm{s})+\mathrm{H}_2 \mathrm{O}({l})

Assume that each astronaut requires

2100 \mathrm{~kcal}

of energy per day. Further assume that this energy is obtained only from the combustion of glucose into

\mathrm{CO}_2(\mathrm{g})

and

\mathrm{H}_2 \mathrm{O}(l).

The standard enthalpies of formation of glucose,

\mathrm{CO}_2

and water are

-1280,-395

and

-285 \mathrm{~kJ} / \mathrm{mol},

respectively. The minimum mass of

\mathrm{LiOH}

required per astronaut per day to react completely with all the

\mathrm{CO}_2

produced is

View answer and explanation

Correct option: A

216 \mathrm{~gm}

Option A (

216 \mathrm{~gm}

) is correct because the calculated minimum mass of LiOH required per astronaut per day is approximately 216 gm.

More Questions from THERMODYNAMICS

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

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

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

0.18 \mathrm{~g}

4 \mathrm{~K}.

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

{CsI}

{CsCl}

{CsCl}

{Cs} I

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

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

\Delta H

\Delta u

\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}