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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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For the reaction 2S + 3O2 > 2SO3 how many grams of O2 will react with 8.12g of sulfur?
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- For the reaction 3KOH+H3PO4⟶K3PO4+3H2O3KOH+H3PO4⟶K3PO4+3H2O how many grams of potassium phosphate, K3PO4, are produced from 44.5 g of potassium hydroxide?arrow_forwardPhosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P4(s) + 5O2(g) -> 2P2O5(g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid H3PO4: P2O5(g) + 3H2O(l) -> 2H3PO4(l) Suppose the yield of the first step is 69.% and the yield of the second step is 82.%. Calculate the mass of phosphorus required to make 1.0kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.arrow_forwardThe combustion of methane is shown in the following reaction:CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) A) If 15.0 moles of CO2(g) is produced, how many moles of methane are required? B) If 20.0 moles of O2(g) are consumed, how many moles of water are produced?arrow_forward
- The molar mass of glucose is 180.2 g/mol. How many grams of glucose will be produced when 132.0g of CO2 reacts with an excess of water?arrow_forward22.0 g of CO2 gas and 9.01 g of H2O gas are formed from combustion of an unknown hydrocarbon (containing only hydrogen and carbon) in the presence of O2 gas. The molar mass of the gas is 84.2 g/mol. What is its molecular formula?arrow_forwardConsider the following balanced chemical reaction: HNO3 + 3H2 → NH2OH + 2H2O If 25.0 grams of HNO3 were mixed with 8.70 grams of H2 gas, how many grams of the excess reagent (i.e. either H2 or HNO3) would remain once the reaction is complete? Molar mass of HNO3 = 63.01 g/mol Molar mass of NH2OH = 33.03 g/molarrow_forward
- N2(g)+3H2(g)--->2NH3(g) If 20.0 moles of ammonia (N H 3) are needed for a particular process, how many moles of diatomic Nitrogen (N 2) are needed?arrow_forwardGiven the following decomposition reaction: 4C3H5O9N3 → O2 + 12CO2 + 10H2O +6N2. a. If 28.40 g H2O were produced, what mass of CO2 will be produced? b. If 110.5 g of C3H5O9N3 were decomposed and the yield of the reaction is 72.3%, determine the theoretical yield and actual yield.arrow_forward
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