Under a high-pressure atmosphere of oxygen, the compound C7H11O4NS2 is burned. A. Write the balanced equation for this reaction. You may assume all the nitrogen is converted to NO2 and the sulfur is converted to SO3. Coefficients should represent the smallest whole number ratio of all reactants and products B- if 77.6 g of the compound is burned, what is the mass of each product?
Under a high-pressure atmosphere of oxygen, the compound C7H11O4NS2 is burned. A. Write the balanced equation for this reaction. You may assume all the nitrogen is converted to NO2 and the sulfur is converted to SO3. Coefficients should represent the smallest whole number ratio of all reactants and products B- if 77.6 g of the compound is burned, what is the mass of each product?
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter4: Stoichiometry
Section: Chapter Questions
Problem 4.71PAE: 4.71 The particulate scale drawing shown depict the products of a reaction between N2 and O2...
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Under a high-pressure atmosphere of oxygen, the compound C7H11O4NS2 is burned.
A. Write the balanced equation for this reaction. You may assume all the nitrogen is converted to NO2 and the sulfur is converted to SO3. Coefficients should represent the smallest whole number ratio of all reactants and products
B- if 77.6 g of the compound is burned, what is the mass of each product?
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