MCQ
For the reaction, $\text{N}_2(\text{g})+3\text{H}_2(\text{g})\rightleftharpoons2\text{NH}_3(\text{g});\ \Delta\text{H}$ is :
- ✓$\Delta\text{U}-2\text{RT}$
- B$\Delta\text{U}-\text{RT}$
- C$\Delta\text{U}+\text{RT}$
- D$\Delta\text{U}+2\text{RT}$
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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 $\left( g\, mol ^{-1}\right):= C =12$