Question

Work the entire problem from the beginning. How many grams of H2 would be formed if 34 grams of carbon reacted with an unlimited amount of H2O? The reaction is: C + H2O → CO + H2 The atomic mass of C is 12.01 g/mole. The atomic mass of H2 is 2.016 g/mole. grams of hydrogen

Answer 1

34 grams of carbon is approx. 2.833 moles(because molar mass of carbon is 12 grams). Since there is unlimited water, Carbon is the limiting reagent, so taking into account that the equation is already balanced and the fact that in the balanced equation the mole ratio between carbon and Hydrogen gas is 1 to 1, there are 2.833 moles of hydrogen, multiply that by the molecular mass of the Hydrogen gas you get 5.71 grams of Hydrogen gas.

Answer 2

Answer: 5.66 g of $H_2$ would be formed if 34 grams of carbon reacted with an unlimited amount of $H_2O$

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}$

$\text{Number of moles of carbon}=\frac{34g}{12g/mol}=2.83moles$

$C+H_2O\rightarrow CO+H_2$

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 $H_2$

Thus 2.83 moles of carbon gives =$\frac{1}{1}\times 2.83=2.83moles$ of $H_2$

Mass of $H_2=moles\times {\text {Molar mass}}=2.83moles\times 2g/mol=5.66g$

Thus 5.66 g of $H_2$ would be formed if 34 grams of carbon reacted with an unlimited amount of $H_2O$