Question

For the reaction CH4 + 202-> CO₂ + 2H₂O, how many moles of water are produced alongside 100g of carbon dioxide.

Answer 1

The number of moles of water produced is 4.54 moles

Step-by-step explanation

Given that:

`\text{ CH}_4\text{ }+2O_2\text{ }\rightarrow\text{ CO}_2\text{ }+\text{ 2H}_2O`

The mass of carbon dioxide is 100g

To find the moles of water, follow the steps below

Step 1: Calculate the moles of carbon dioxide using the formula below

`\text{ Mole }=\text{ }\frac{\text{ mass}}{molar\text{ mass}}`

Recall, that the molar mass of CO2 is 44.01 g/ mol

Step 2: Substitute the given data into the formula in step 1

`\begin{gathered} \text{ mole }=\text{ }(100)/(44.01) \\ \text{ mole }=2.272\text{ moles} \end{gathered}`

Step 3: Find the moles of water produced using a stoichiometry ratio

In the reaction above, 1 mole of CO2 is equivalent to 2 moles of H2O

Let x represent the number of moles of water

`\begin{gathered} \text{ 1 mole CO}_2\text{ }\rightarrow\text{ 2 moles H}_2O \\ \text{ 2.272 moles CO}_2\text{ }\rightarrow\text{ x moles H}_2O \\ \text{ Cross multiply} \\ \text{ 1 mole CO}_2\text{ }*\text{ x moles H}_2O\text{ }=\text{ 2 moles H}_2O*2.272\text{ moles CO}_2 \\ \text{ Isolate x} \\ \text{ x }=\frac{2\text{ moles H}_2O*2.272\cancel{molesCO_2}}{1\cancel{moleCO_2}} \\ \text{ x }=\text{ 2 }*\text{ 2.272} \\ \text{ x }=\text{ 4.54 moles} \end{gathered}`

Therefore, the number of moles of water produced is 4.54 moles