Discover the best answers at Westonci.ca, where experts share their insights and knowledge with you. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform.
Sagot :
Certainly! Let's solve this step-by-step.
1. Identify the Given Reaction and Known Quantities:
The balanced chemical equation provided is:
[tex]\[ 2 \, C_6H_6(g) + 15 \, O_2(g) \rightarrow 12 \, CO_2(g) + 6 \, H_2O(g) \][/tex]
We are given that 2.00 moles of [tex]\(C_6H_6\)[/tex] reacts with oxygen.
2. Identify the Relevant Stoichiometric Ratios:
According to the balanced chemical equation, 2 moles of [tex]\(C_6H_6\)[/tex] produce 6 moles of [tex]\(H_2O\)[/tex]. This can be written as a stoichiometric ratio:
[tex]\[ \frac{6 \, \text{mol} \, H_2O}{2 \, \text{mol} \, C_6H_6} \][/tex]
3. Calculate the Moles of [tex]\(H_2O\)[/tex] Produced:
Since we start with 2.00 moles of [tex]\(C_6H_6\)[/tex]:
[tex]\[ \text{Moles of } H_2O = \left( \frac{6 \, \text{mol} \, H_2O}{2 \, \text{mol} \, C_6H_6} \right) \times 2.00 \, \text{mol} \, C_6H_6 \][/tex]
Simplifying the expression, we get:
[tex]\[ \text{Moles of } H_2O = 6.00 \, \text{mol} \][/tex]
4. Convert Moles of [tex]\(H_2O\)[/tex] to Volume at STP:
At Standard Temperature and Pressure (STP), 1 mole of any ideal gas occupies 22.4 liters. Therefore, we can find the volume of water vapor produced using the number of moles calculated:
[tex]\[ \text{Volume of } H_2O = 6.00 \, \text{mol} \times 22.4 \, \text{L/mol} \][/tex]
Simplifying this, we obtain:
[tex]\[ \text{Volume of } H_2O = 134.4 \, \text{L} \][/tex]
Thus, the volume of water vapor produced at STP is [tex]\(134.4 \, \text{liters}\)[/tex].
1. Identify the Given Reaction and Known Quantities:
The balanced chemical equation provided is:
[tex]\[ 2 \, C_6H_6(g) + 15 \, O_2(g) \rightarrow 12 \, CO_2(g) + 6 \, H_2O(g) \][/tex]
We are given that 2.00 moles of [tex]\(C_6H_6\)[/tex] reacts with oxygen.
2. Identify the Relevant Stoichiometric Ratios:
According to the balanced chemical equation, 2 moles of [tex]\(C_6H_6\)[/tex] produce 6 moles of [tex]\(H_2O\)[/tex]. This can be written as a stoichiometric ratio:
[tex]\[ \frac{6 \, \text{mol} \, H_2O}{2 \, \text{mol} \, C_6H_6} \][/tex]
3. Calculate the Moles of [tex]\(H_2O\)[/tex] Produced:
Since we start with 2.00 moles of [tex]\(C_6H_6\)[/tex]:
[tex]\[ \text{Moles of } H_2O = \left( \frac{6 \, \text{mol} \, H_2O}{2 \, \text{mol} \, C_6H_6} \right) \times 2.00 \, \text{mol} \, C_6H_6 \][/tex]
Simplifying the expression, we get:
[tex]\[ \text{Moles of } H_2O = 6.00 \, \text{mol} \][/tex]
4. Convert Moles of [tex]\(H_2O\)[/tex] to Volume at STP:
At Standard Temperature and Pressure (STP), 1 mole of any ideal gas occupies 22.4 liters. Therefore, we can find the volume of water vapor produced using the number of moles calculated:
[tex]\[ \text{Volume of } H_2O = 6.00 \, \text{mol} \times 22.4 \, \text{L/mol} \][/tex]
Simplifying this, we obtain:
[tex]\[ \text{Volume of } H_2O = 134.4 \, \text{L} \][/tex]
Thus, the volume of water vapor produced at STP is [tex]\(134.4 \, \text{liters}\)[/tex].
We hope you found this helpful. Feel free to come back anytime for more accurate answers and updated information. We appreciate your time. Please revisit us for more reliable answers to any questions you may have. We're glad you visited Westonci.ca. Return anytime for updated answers from our knowledgeable team.