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$Fe _{3} O _{4}( s )+4 CO ( g ) \rightarrow 3 Fe ( l )+4 CO _{2}( g )$
when $4.640 \,kg$ of $Fe _{3} O _{4}$ and $2.520 \,kg$ of $CO$ are allowed to react then the amount of iron (in $g$ ) produced is $....$
[Given : Molar Atomic mass $\left( g\, mol ^{-1}\right): Fe =56$
Molar Atomic mass $\left( g \,mol ^{-1}\right): 0=16$
Molar Atomic mass $\left( g\, mol ^{-1}\right):= C =12$
$[{N_2}{O_4}\,(g)\, \rightleftharpoons \,2N{o_2}(g)]$
At $300\,K$ and $1\,atm$ pressure, the degree of dissociation of $N_2O_4$ is $0.2.$ If one mole of $N_2O_4$ gas is contained in a vessel, then the density of the equilibrium mixture is.......$g/L$
$' A ^{\prime} \stackrel{ HNO _3}{\longrightarrow} X ^{\prime} \stackrel{ NaBH _4}{\longrightarrow} \underset{\text { Chiral compound }}{\text { } B ^{}}$ $X$ is $.......$.
${C_{(gr)}} + {O_{2(g)}} \to C{O_{2(g)}}\,\,\,\Delta H = x\,kJ/mol$
${C_{(gr)}} + \frac{1}{2}{O_{2(g)}} \to C{O_{(g)}}\,\,\,\Delta H = y\,kJ/mol$
$C{O_{(g)}} + \frac{1}{2}{O_{2(g)}} \to C{O_2}_{(g)}\,\,\,\Delta H = z\,kJ/mol$