Answer :
To determine how many grams of [tex]\( H_2O \)[/tex] can be formed from [tex]\( 5.58 \, \text{g} \, H_2 \)[/tex], we can follow these steps:
1. Understand the chemical equation:
The balanced equation is:
[tex]\[
2 H_2(g) + O_2(g) \longrightarrow 2 H_2O(g)
\][/tex]
This shows that 2 moles of [tex]\( H_2 \)[/tex] produce 2 moles of [tex]\( H_2O \)[/tex].
2. Calculate the molar masses:
- The molar mass of [tex]\( H_2 \)[/tex] is approximately [tex]\( 2.016 \, \text{g/mol} \)[/tex].
- The molar mass of [tex]\( H_2O \)[/tex] is approximately [tex]\( 18.015 \, \text{g/mol} \)[/tex].
3. Convert grams of [tex]\( H_2 \)[/tex] to moles:
To find out how many moles of [tex]\( H_2 \)[/tex] are in 5.58 grams, use the molar mass:
[tex]\[
\text{moles of } H_2 = \frac{5.58 \, \text{g}}{2.016 \, \text{g/mol}} \approx 2.768 \, \text{moles}
\][/tex]
4. Use the stoichiometry of the equation:
According to the equation, the moles of [tex]\( H_2 \)[/tex] and [tex]\( H_2O \)[/tex] are in a 1:1 ratio. Thus, 2.768 moles of [tex]\( H_2 \)[/tex] will produce 2.768 moles of [tex]\( H_2O \)[/tex].
5. Convert moles of [tex]\( H_2O \)[/tex] to grams:
Multiply the moles of [tex]\( H_2O \)[/tex] by its molar mass to find the grams:
[tex]\[
\text{mass of } H_2O = 2.768 \, \text{moles} \times 18.015 \, \text{g/mol} \approx 49.9 \, \text{g}
\][/tex]
Therefore, from 5.58 grams of [tex]\( H_2 \)[/tex], approximately 49.9 grams of [tex]\( H_2O \)[/tex] can be formed. The correct answer is 49.9 g.
1. Understand the chemical equation:
The balanced equation is:
[tex]\[
2 H_2(g) + O_2(g) \longrightarrow 2 H_2O(g)
\][/tex]
This shows that 2 moles of [tex]\( H_2 \)[/tex] produce 2 moles of [tex]\( H_2O \)[/tex].
2. Calculate the molar masses:
- The molar mass of [tex]\( H_2 \)[/tex] is approximately [tex]\( 2.016 \, \text{g/mol} \)[/tex].
- The molar mass of [tex]\( H_2O \)[/tex] is approximately [tex]\( 18.015 \, \text{g/mol} \)[/tex].
3. Convert grams of [tex]\( H_2 \)[/tex] to moles:
To find out how many moles of [tex]\( H_2 \)[/tex] are in 5.58 grams, use the molar mass:
[tex]\[
\text{moles of } H_2 = \frac{5.58 \, \text{g}}{2.016 \, \text{g/mol}} \approx 2.768 \, \text{moles}
\][/tex]
4. Use the stoichiometry of the equation:
According to the equation, the moles of [tex]\( H_2 \)[/tex] and [tex]\( H_2O \)[/tex] are in a 1:1 ratio. Thus, 2.768 moles of [tex]\( H_2 \)[/tex] will produce 2.768 moles of [tex]\( H_2O \)[/tex].
5. Convert moles of [tex]\( H_2O \)[/tex] to grams:
Multiply the moles of [tex]\( H_2O \)[/tex] by its molar mass to find the grams:
[tex]\[
\text{mass of } H_2O = 2.768 \, \text{moles} \times 18.015 \, \text{g/mol} \approx 49.9 \, \text{g}
\][/tex]
Therefore, from 5.58 grams of [tex]\( H_2 \)[/tex], approximately 49.9 grams of [tex]\( H_2O \)[/tex] can be formed. The correct answer is 49.9 g.
