Combustion of octane (regular gasoline): 2 C3H18 + 25 O2 → 16 CO2 + 18 H20 How many grams of CO2 are produced from burning 2.0 x 103 grams of octane. What is the 2nd step you would take? B Take grams of carbon dioxide and multiply by the molar mass of carbon dioxide to get moles of carbon dioxide Take grams of octane and divide by molar mass of carbon dioxide. D Convert moles of octane to moles of carbon dioxide using the molar ratio Take grams of octane and divide by the molar mass of octane to get moles of octane

Combustion of octane (regular gasoline): 2 C3H18 + 25 O2 → 16 CO2 + 18 H20 How many grams of CO2 are produced from burning 2.0 x 103 grams of octane. What is the 2nd step you would take? B Take grams of carbon dioxide and multiply by the molar mass of carbon dioxide to get moles of carbon dioxide Take grams of octane and divide by molar mass of carbon dioxide. D Convert moles of octane to moles of carbon dioxide using the molar ratio Take grams of octane and divide by the molar mass of octane to get moles of octane

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

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 114E: a. Write die balanced equation for the combustion of isooctane (C8H18) to produce water vapor and...

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3.81 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients.
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
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ou know that chemical A reacts with chemical B. You react 10.0 g A with 10.0 g B. What information do you need to know to determine the amount of product that will be produced? Explain.