Question

Use the problem below to answer the question: 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 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

Answer 1

34g C * ( 1 mol / 12.0107 ) * ( 1 mol H2 / 1 mol C ) * ( 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 using the given amount of grams and the molar mass ( 2.01588 g/mol ).

Revise your answer to have the correct number of significant figures.

Answer 2

Answer: The mass of hydrogen gas formed will be 5.66 g

Step-by-step explanation:

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

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

For Carbon:

Given mass = 34 g

Molar mass = 12 g/mol

Putting values in above equation, we get:

`\text{Moles of carbon}=(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 =
`(1)/(1)* 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