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 – no fractional coefficients. (7.5 pts.)
B. If 77.6 g of the compound is burned, what is the mass of
each product?
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Under a high-pressure atmosphere of oxygen, the compound C7H11O4NS2 is burned A. Write the balanced equation...
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