Answered

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. Finish the problem by choosing the correct format for dimensional analysis.

Verified Answer :

Equation: 
C + H2O → CO + H2 
1mol C produces 1 mol H2 
Molar mass Co = 12.01g/mol 
mol C in 34g = 34/12.01 = 2.831 mol of C 
This will produce 2.831 mol H2 
Molar mass H2 = 2016 g/mol 
Mass of 2.831 mol H2 = 2.831 * 2.016 = 5.7072g H2 produced 
Answer must have 2 significant figures: Mass H2 = 5.7g

Answer : The mass of \(H_2\) will be, 5.66 grams

Explanation : Given,

Mass of C = 34 g

Molar mass of C = 12 g/mole

Molar mass of \(H_2\) = 2 g/mole

First we have to calculate the moles of carbon.

\(\text{Moles of }C=\frac{\text{Mass of }C}{\text{Molar mass of }C}=\frac{34g}{12g/mole}=2.83mole\)

Now we have to calculate the moles of \(H_2\).

The given balanced chemical reaction is,

\(C+H_2O\rightarrow CO+H_2\)

From the balanced reaction, we conclude that

As, 1 mole of C react to give 1 mole of \(H_2\)

So, 2.83 mole of C react to give 2.83 mole of \(H_2\)

Now we have to calculate the mass of \(H_2\).

\(\text{Mass of }H_2=\text{Moles of }H_2\times \text{Molar mass of }H_2=2.83mole\times 2=5.66g\)

Therefore, the mass of \(H_2\) will be, 5.66 grams

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