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Wewaii [24]
3 years ago
5

Use the problem below to answer the question: How many grams of H2 would be formed if 34 grams of carbon reacted with an unlimit

ed amount of H2O? The reaction is: C + H2O → CO + H2 The equation is balanced. The starting substance is carbon, C. The ending substance is hydrogen, H2. Using the periodic table, find the molecular mass of H2. H2 = g/mole
Chemistry
2 answers:
Pavlova-9 [17]3 years ago
6 0
34g C * ( 1 mol / 12.0107 ) * ( 1 mol H2 / 1 mol C ) * ( <span>2.01588 g / 1 mol H2 ) = 5.70657164028741 g H2 = 5.7 g H2

Convert grams of C to moles of C using the given amount of grams and the molar mass ( 12.0107 g/mol ).

Gather the mole ratio from the coefficients in the balanced equation and multiply by the ratio.

Convert moles of H2 to grams of H2 </span> using the given amount of grams and the molar mass ( 2.01588 g/mol )<span>.

Revise your answer to have the correct number of significant figures. </span>
Aleksandr [31]3 years ago
5 0

<u>Answer:</u> The mass of hydrogen gas formed will be 5.66 g

<u>Explanation:</u>

To calculate the number of moles, we use the formula:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}    .....(1)

<u>For Carbon:</u>

Given mass = 34 g

Molar mass = 12 g/mol

Putting values in above equation, we get:

\text{Moles of carbon}=\frac{34g}{12g/mol}=2.83mol

For the given chemical equation:

C+H_2O\rightarrow CO+H_2

By Stoichiometry of the reaction:

1 mole of carbon produces 1 mole of hydrogen gas.

So, 2.83 moles of carbon atom will produce = \frac{1}{1}\times 2.83=2.83mol of hydrogen gas.

Now, to calculate the mass of hydrogen gas, we use equation 1.

Moles of Hydrogen gas = 2.83 mol

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1, we get:

2.83mol=\frac{\text{Mass of Hydrogen gas}}{2g/mol}\\\\\text{Mass of Hydrogen gas}=5.66g

Hence, the mass of hydrogen gas formed will be 5.66 g

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