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Answer :
We start with the balanced chemical equation:
[tex]$$
2 H_2 + O_2 \rightarrow 2 H_2O
$$[/tex]
Step 1: Determine the mole ratio
The equation shows that 2 moles of hydrogen gas ([tex]$H_2$[/tex]) produce 2 moles of water ([tex]$H_2O$[/tex]). This means the mole ratio between [tex]$H_2$[/tex] and [tex]$H_2O$[/tex] is 1:1. Therefore, if you have 6.00 moles of [tex]$H_2$[/tex], you will produce 6.00 moles of [tex]$H_2O$[/tex].
Step 2: Calculate the molar mass of water
Using the periodic table:
- Atomic mass of hydrogen, [tex]$H \approx 1.01\ \text{g/mol}$[/tex]
- Atomic mass of oxygen, [tex]$O \approx 16.00\ \text{g/mol}$[/tex]
Water, [tex]$H_2O$[/tex], contains 2 hydrogen atoms and 1 oxygen atom, so its molar mass is:
[tex]$$
M(H_2O) = 2(1.01\ \text{g/mol}) + 16.00\ \text{g/mol} = 2.02\ \text{g/mol} + 16.00\ \text{g/mol} = 18.02\ \text{g/mol}.
$$[/tex]
Step 3: Calculate the mass of water produced
Now, multiply the number of moles of water by its molar mass:
[tex]$$
\text{Mass of } H_2O = 6.00\ \text{mol} \times 18.02\ \text{g/mol} = 108.12\ \text{g}.
$$[/tex]
Thus, approximately [tex]$108\ \text{g}$[/tex] of water are produced.
Final Answer: Option D: [tex]$108\ \text{g}$[/tex].
[tex]$$
2 H_2 + O_2 \rightarrow 2 H_2O
$$[/tex]
Step 1: Determine the mole ratio
The equation shows that 2 moles of hydrogen gas ([tex]$H_2$[/tex]) produce 2 moles of water ([tex]$H_2O$[/tex]). This means the mole ratio between [tex]$H_2$[/tex] and [tex]$H_2O$[/tex] is 1:1. Therefore, if you have 6.00 moles of [tex]$H_2$[/tex], you will produce 6.00 moles of [tex]$H_2O$[/tex].
Step 2: Calculate the molar mass of water
Using the periodic table:
- Atomic mass of hydrogen, [tex]$H \approx 1.01\ \text{g/mol}$[/tex]
- Atomic mass of oxygen, [tex]$O \approx 16.00\ \text{g/mol}$[/tex]
Water, [tex]$H_2O$[/tex], contains 2 hydrogen atoms and 1 oxygen atom, so its molar mass is:
[tex]$$
M(H_2O) = 2(1.01\ \text{g/mol}) + 16.00\ \text{g/mol} = 2.02\ \text{g/mol} + 16.00\ \text{g/mol} = 18.02\ \text{g/mol}.
$$[/tex]
Step 3: Calculate the mass of water produced
Now, multiply the number of moles of water by its molar mass:
[tex]$$
\text{Mass of } H_2O = 6.00\ \text{mol} \times 18.02\ \text{g/mol} = 108.12\ \text{g}.
$$[/tex]
Thus, approximately [tex]$108\ \text{g}$[/tex] of water are produced.
Final Answer: Option D: [tex]$108\ \text{g}$[/tex].
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