Consider the following reaction occurring in the blast furnace: $Fe_3O_{4(s)} + 4CO_{(g)} \rightarrow 3Fe_{(l)} + 4CO_{2(g)}$. '$x$' kg of iron is produced when $2.32 \times 10^3 \ kg$ of $Fe_3O_4$ and $2.8 \times 10^2 \ kg$ of $CO$ are brought together in the furnace. The value of '$x$' is $.............$ (nearest integer). Given: Molar mass of $Fe_3O_4 = 232 \ g \ mol^{-1}$,Molar mass of $CO = 28 \ g \ mol^{-1}$,Molar mass of $Fe = 56 \ g \ mol^{-1}$.
- A$420$
- B$320$
- C$220$
- D$250$
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Similar Questions
Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation:
$N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$
$(i)$ Calculate the mass of ammonia produced if $2.00 \times 10^{3} \, g$ of dinitrogen reacts with $1.00 \times 10^{3} \, g$ of dihydrogen.
$(ii)$ Will any of the two reactants remain unreacted?
$(iii)$ If yes,which one and what would be its mass?
$N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$
$(i)$ Calculate the mass of ammonia produced if $2.00 \times 10^{3} \, g$ of dinitrogen reacts with $1.00 \times 10^{3} \, g$ of dihydrogen.
$(ii)$ Will any of the two reactants remain unreacted?
$(iii)$ If yes,which one and what would be its mass?
Medium
View SolutionWhat volume of hydrogen gas at $STP$ would be liberated by the action of $50 \text{ mL}$ of $H_2SO_4$ of $50\%$ purity (density = $1.3 \text{ g mL}^{-1}$) on $20 \text{ g}$ of zinc (in $L$)? Given: Molar mass of $H, O, S, Zn$ are $1, 16, 32, 65 \text{ g mol}^{-1}$ respectively.
DifficultJEE MAIN 2026
View SolutionThe mass of ammonia in grams produced when $2.8 \ kg$ of dinitrogen quantitatively reacts with $1 \ kg$ of dihydrogen is.............
For the gaseous reaction $H_2 + Cl_2 \rightarrow 2HCl$,if $20 \ mL$ of $H_2$ and $30 \ mL$ of $Cl_2$ are taken initially,the volume of $HCl$ formed and the volume of unreacted $Cl_2$ are respectively .....
Medium
View Solution$CaCO_{3(s)} + 2 HCl_{(aq)} \rightarrow CaCl_{2(aq)} + CO_{2(g)} + H_2O_{(l)}$
Consider the above reaction,what mass of $CaCl_2$ will be formed if $250 \ mL$ of $0.76 \ M \ HCl$ reacts with $1000 \ g$ of $CaCO_3$ (in $g$)?
(Given: Molar mass of $Ca, C, O, H$ and $Cl$ are $40, 12, 16, 1$ and $35.5 \ g \ mol^{-1}$,respectively)
Consider the above reaction,what mass of $CaCl_2$ will be formed if $250 \ mL$ of $0.76 \ M \ HCl$ reacts with $1000 \ g$ of $CaCO_3$ (in $g$)?
(Given: Molar mass of $Ca, C, O, H$ and $Cl$ are $40, 12, 16, 1$ and $35.5 \ g \ mol^{-1}$,respectively)
DifficultJEE MAIN 2025
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