Answer: 5.66 g of [tex]H_2[/tex] would be formed if 34 grams of carbon reacted with an unlimited amount of [tex]H_2O[/tex]
Explanation:
According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number [tex]6.023\times 10^{23}[/tex] of particles.
To calculate the moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}[/tex]
[tex]\text{Number of moles of carbon}=\frac{34g}{12g/mol}=2.83moles[/tex]
[tex]C+H_2O\rightarrow CO+H_2[/tex]
Carbon is the limiting reagent as it limits the formation of product and hydrogen is the excess reagent.
According to stoichiometry :
1 mole of carbon gives = 1 mole of [tex]H_2[/tex]
Thus 2.83 moles of carbon gives =[tex]\frac{1}{1}\times 2.83=2.83moles[/tex] of [tex]H_2[/tex]
Mass of [tex]H_2=moles\times {\text {Molar mass}}=2.83moles\times 2g/mol=5.66g[/tex]
Thus 5.66 g of [tex]H_2[/tex] would be formed if 34 grams of carbon reacted with an unlimited amount of [tex]H_2O[/tex]
