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 What substance are we expected to solve for?

Answer 1

Answer : The mass of hydrogen gas
`H_2` will be, 5.6 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 (C).

`\text{Moles of }C=\frac{\text{Mass of }C}{\text{Molar mass of }C}=(34g)/(12g/mole)=2.8moles`

Now we have to calculate the moles of
`H_2`.

The 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, 2.8 moles of
`C` react to give 2.8 moles of
`H_2`

Now we have to calculate the mass of
`H_2`.

`\text{Mass of }H_2=\text{Moles of }H_2* \text{Molar mass of }H_2`

`\text{Mass of }H_2=(2.8mole)* (2g/mole)=5.6g`

Therefore, the mass of hydrogen gas
`H_2` will be, 5.6 grams.

Answer 2

You have to find how many moles of H2 has formed.

C+ H2O -> CO + H2

mole of carbon reacted = mass / molar mass = 34g/ 12g per mol = 2.83 mol

for every 1 mole of carbon will form 1 mole of H2

mole of hydrogen produced = 1* 2.83 = 2.83 mol

mass of hydrogen = mole * molar mass = 2.83 mol * (1*2) = 5.66g