The balanced equation for the decomposition of ammonium nitrate is 2NH4NO3(s) → 2N2(g) + O2(g) + 4H2O(g) (a) Select the mole ratios that relate moles of each product to the reactant NH4NO3. 2 mol NH4NO3 2 mol N2 2 mol N2 2 mol NH4NO3 2 mol NH4NO3 1 mol O2 1 mol O2 2 mol NH4NO3 2 mol NH4NO3 4 mol H2O 4 mol H2O 2 mol NH4NO3 (b) How many moles of each product would form if 1.00 mol of NH4NO3 reacts? Moles of N2 = mol N2 Moles of O2 = mol O2 Moles of H2O = mol H2O (c) How many moles of each product would form if 9.74 mol of NH4NO3 react? Moles of N2 = mol N2 Moles of O2 = mol O2 Moles of H2O = mol H2O
The balanced equation for the decomposition of ammonium nitrate is 2NH4NO3(s) → 2N2(g) + O2(g) + 4H2O(g) (a) Select the mole ratios that relate moles of each product to the reactant NH4NO3. 2 mol NH4NO3 2 mol N2 2 mol N2 2 mol NH4NO3 2 mol NH4NO3 1 mol O2 1 mol O2 2 mol NH4NO3 2 mol NH4NO3 4 mol H2O 4 mol H2O 2 mol NH4NO3 (b) How many moles of each product would form if 1.00 mol of NH4NO3 reacts? Moles of N2 = mol N2 Moles of O2 = mol O2 Moles of H2O = mol H2O (c) How many moles of each product would form if 9.74 mol of NH4NO3 react? Moles of N2 = mol N2 Moles of O2 = mol O2 Moles of H2O = mol H2O
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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The balanced equation for the decomposition of ammonium nitrate is
(a) Select the mole ratios that relate moles of each product to the reactant NH4NO3.
(b) How many moles of each product would form if 1.00 mol of NH4NO3 reacts?
(c) How many moles of each product would form if 9.74 mol of NH4NO3 react?
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