To determine the number of moles of [tex]\( H_2O \)[/tex] formed from a given amount of [tex]\( C_2H_4 \)[/tex], let's follow these step-by-step instructions:
1. Write the balanced equation:
[tex]\[
C_2H_4(g) + 3O_2(g) \rightarrow 2CO_2(g) + 2H_2O(g)
\][/tex]
2. Identify the stoichiometric relationship between [tex]\(C_2H_4\)[/tex] and [tex]\(H_2O\)[/tex]:
According to the balanced equation, 1 mole of [tex]\( C_2H_4 \)[/tex] produces 2 moles of [tex]\( H_2O \)[/tex].
3. Given information:
The number of moles of [tex]\( C_2H_4 \)[/tex] is 0.60 moles.
4. Use stoichiometry to find the moles of [tex]\( H_2O \)[/tex]:
Since 1 mole of [tex]\( C_2H_4 \)[/tex] produces 2 moles of [tex]\( H_2O \)[/tex], multiply the moles of [tex]\( C_2H_4 \)[/tex] by the stoichiometric factor (2 moles [tex]\( H_2O \)[/tex] per 1 mole [tex]\( C_2H_4 \)[/tex]):
[tex]\[
\text{Moles of } H_2O = 0.60 \, \text{moles of } C_2H_4 \times \frac{2 \, \text{moles of } H_2O}{1 \, \text{mole of } C_2H_4}
\][/tex]
[tex]\[
\text{Moles of } H_2O = 0.60 \times 2 = 1.2 \, \text{moles}
\][/tex]
5. Adjust for significant figures:
The initial moles of [tex]\( C_2H_4 \)[/tex] (0.60) have two significant figures. Therefore, the final answer should also be reported with two significant figures.
Thus, the number of moles of [tex]\( H_2O \)[/tex] formed from 0.60 moles of [tex]\( C_2H_4 \)[/tex] is:
[tex]\[
\boxed{1.2 \, \text{moles} \, H_2O}
\][/tex]
