228339 Production of iron in blast furnace follows the following equation:
$\mathrm{Fe}_3 \mathrm{O}_4(\mathrm{~s})+4 \mathrm{CO}(\mathrm{g}) \rightarrow 3 \mathrm{Fe}(1)+4 \mathrm{CO}_2(\mathrm{~g})$
When $4.640 \mathrm{~kg}$ of $\mathrm{Fe}_3 \mathrm{O}_4$ and $2.520 \mathrm{~kg}$ of $\mathrm{CO}$ are allowed to react then the amount of iron (in g) produced is:
[Given: Molar Atomic mass $\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathrm{Fe}=$ 56
Molar Atomic mass $\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathbf{O}=16$
Molar Atomic mass $\left.\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathrm{C}=12\right]$

228340 The maximum number of molecules is present in

228341 $10 \mathrm{gm}$ of hydrogen and $64 \mathrm{~g}$ of oxygen were kept in a steel vessel and exploded. Amount of water produced in this reaction will be

228342 The mass of one mole of electron is

228339 Production of iron in blast furnace follows the following equation:
$\mathrm{Fe}_3 \mathrm{O}_4(\mathrm{~s})+4 \mathrm{CO}(\mathrm{g}) \rightarrow 3 \mathrm{Fe}(1)+4 \mathrm{CO}_2(\mathrm{~g})$
When $4.640 \mathrm{~kg}$ of $\mathrm{Fe}_3 \mathrm{O}_4$ and $2.520 \mathrm{~kg}$ of $\mathrm{CO}$ are allowed to react then the amount of iron (in g) produced is:
[Given: Molar Atomic mass $\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathrm{Fe}=$ 56
Molar Atomic mass $\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathbf{O}=16$
Molar Atomic mass $\left.\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathrm{C}=12\right]$

228340 The maximum number of molecules is present in

228341 $10 \mathrm{gm}$ of hydrogen and $64 \mathrm{~g}$ of oxygen were kept in a steel vessel and exploded. Amount of water produced in this reaction will be

228342 The mass of one mole of electron is

228339 Production of iron in blast furnace follows the following equation:
$\mathrm{Fe}_3 \mathrm{O}_4(\mathrm{~s})+4 \mathrm{CO}(\mathrm{g}) \rightarrow 3 \mathrm{Fe}(1)+4 \mathrm{CO}_2(\mathrm{~g})$
When $4.640 \mathrm{~kg}$ of $\mathrm{Fe}_3 \mathrm{O}_4$ and $2.520 \mathrm{~kg}$ of $\mathrm{CO}$ are allowed to react then the amount of iron (in g) produced is:
[Given: Molar Atomic mass $\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathrm{Fe}=$ 56
Molar Atomic mass $\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathbf{O}=16$
Molar Atomic mass $\left.\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathrm{C}=12\right]$

228340 The maximum number of molecules is present in

228341 $10 \mathrm{gm}$ of hydrogen and $64 \mathrm{~g}$ of oxygen were kept in a steel vessel and exploded. Amount of water produced in this reaction will be

228342 The mass of one mole of electron is

228339 Production of iron in blast furnace follows the following equation:
$\mathrm{Fe}_3 \mathrm{O}_4(\mathrm{~s})+4 \mathrm{CO}(\mathrm{g}) \rightarrow 3 \mathrm{Fe}(1)+4 \mathrm{CO}_2(\mathrm{~g})$
When $4.640 \mathrm{~kg}$ of $\mathrm{Fe}_3 \mathrm{O}_4$ and $2.520 \mathrm{~kg}$ of $\mathrm{CO}$ are allowed to react then the amount of iron (in g) produced is:
[Given: Molar Atomic mass $\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathrm{Fe}=$ 56
Molar Atomic mass $\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathbf{O}=16$
Molar Atomic mass $\left.\left(\mathrm{g} \mathrm{mol}^{-1}\right): \mathrm{C}=12\right]$

228340 The maximum number of molecules is present in

228341 $10 \mathrm{gm}$ of hydrogen and $64 \mathrm{~g}$ of oxygen were kept in a steel vessel and exploded. Amount of water produced in this reaction will be

228342 The mass of one mole of electron is