A complete combustion of octane, C8H18, a component of gasoline, proceeds as: C8H18(l ) + O2(g) → CO2(g) + H2O(l) {unbalanced equation} Atomic weights (g/mol): C=12, H=1, O=16 500 grams of oxygen is made to react with an excess amount of octane. What is the percent yield if 312 grams of carbon dioxide is actually produced? Enter final answer with TWO decimal places (e.g. 37.18 or 35.00 or 98.20); numeric answers only, do not include the units.
A complete combustion of octane, C8H18, a component of gasoline, proceeds as: C8H18(l ) + O2(g) → CO2(g) + H2O(l) {unbalanced equation} Atomic weights (g/mol): C=12, H=1, O=16 500 grams of oxygen is made to react with an excess amount of octane. What is the percent yield if 312 grams of carbon dioxide is actually produced? Enter final answer with TWO decimal places (e.g. 37.18 or 35.00 or 98.20); numeric answers only, do not include the units.
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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A complete combustion of octane, C8H18, a component of gasoline, proceeds as: C8H18(l ) + O2(g) → CO2(g) + H2O(l) {unbalanced equation}
Atomic weights (g/mol): C=12, H=1, O=16
500 grams of oxygen is made to react with an excess amount of octane. What is the percent yield if 312 grams of carbon dioxide is actually produced? Enter final answer with TWO decimal places (e.g. 37.18 or 35.00 or 98.20); numeric answers only, do not include the units.
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