What is the mass in grams of CO, that can be produced from the combustion of 2.76 moles 2 of butane according to this equation: 2 C,H1,(g) + 13 0,(g) → 8 CO2(g) + 10 H,0(g)
What is the mass in grams of CO, that can be produced from the combustion of 2.76 moles 2 of butane according to this equation: 2 C,H1,(g) + 13 0,(g) → 8 CO2(g) + 10 H,0(g)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Combustion of Butane: Calculating CO₂ Mass**
**Question:**
What is the mass in grams of CO₂ that can be produced from the combustion of 2.76 moles of butane according to this equation?
**Chemical Equation:**
\[ 2 \, \text{C}_4\text{H}_{10}(g) + 13 \, \text{O}_2(g) \rightarrow 8 \, \text{CO}_2(g) + 10 \, \text{H}_2\text{O}(g) \]
**Analysis:**
To find the answer, we use stoichiometry based on the balanced chemical equation. The equation shows that 2 moles of butane (\(\text{C}_4\text{H}_{10}\)) produce 8 moles of carbon dioxide (\(\text{CO}_2\)). Using the given 2.76 moles of butane, we can calculate the moles of \(\text{CO}_2\) produced and then determine its mass in grams.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F49444d66-96b7-45b8-992f-0f6c51b0e4d0%2F82f36e0e-5d8c-4965-80aa-764078f2c169%2Fv4kroyd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Combustion of Butane: Calculating CO₂ Mass**
**Question:**
What is the mass in grams of CO₂ that can be produced from the combustion of 2.76 moles of butane according to this equation?
**Chemical Equation:**
\[ 2 \, \text{C}_4\text{H}_{10}(g) + 13 \, \text{O}_2(g) \rightarrow 8 \, \text{CO}_2(g) + 10 \, \text{H}_2\text{O}(g) \]
**Analysis:**
To find the answer, we use stoichiometry based on the balanced chemical equation. The equation shows that 2 moles of butane (\(\text{C}_4\text{H}_{10}\)) produce 8 moles of carbon dioxide (\(\text{CO}_2\)). Using the given 2.76 moles of butane, we can calculate the moles of \(\text{CO}_2\) produced and then determine its mass in grams.
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