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Interpretation:
The limiting reactant when
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INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN
- One way to remove nitrogen oxide (NO) from smoke-stack emissions is to react it with ammonia. 4NH3(g)+6NO(g)5N2(g)+6H2O(l) Calculate (a) the mass of water produced from 0.839 mol of ammonia. (b) the mass of NO required to react with 3.402 mol of ammonia. (c) the mass of ammonia required to produce 12.0 g of nitrogen gas. (d) the mass of ammonia required to react with 115 g of NO.arrow_forwardAccording to the following equation, how many moles of oxygen gas are produced from the decomposition of 3.0 mol of Al2O3? (Assume an 85% ) 2 Al2O3 → 4 Al + 3O2arrow_forwardGlucose, C6H12O6,C6H12O6, is used as an energy source by the human body. The overall reaction in the body is described by the equation C6H12O6(aq)+6O2(g)⟶6CO2(g)+6H2O(l) Calculate the number of grams of oxygen required to convert 53.0 g of glucose to CO2arrow_forward
- Determine the grams of ammonia produced when 1.15 g of hydrogen H is reacted with 3.75 g of nitrogen N to produce ammonia (NH) according to the following chemical equation: 3H + N → 2NHarrow_forwardGiven the following reaction: 2 C2H6(l) + 7 O2(g) => 4 CO2(g) + 6 H2O(l) How many moles of water are produced when 3.0 moles of oxygen react?arrow_forwardEthylene burns in oxygen to form carbon dioxide and water vapor at the same temperature and pressure according to this equation - C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(g) How many liters of water can be formed if 1.25 liters of ethylene are consumed in this reaction?arrow_forward
- How many grams of Na2O are produced when 72.6 g of Na reacts?arrow_forwardGiven the chemical equation: 2H₂ + O₂ → 2H₂O, how many moles of H₂O is produced to balance the equation?arrow_forwardGiven: 2KClO3(s) 2KCl + 3O2(g) How many grams of oxygen are produced by the decomposition of 1.70 moles of potassiumchlorate?arrow_forward
- For the reaction represented by the equation 2H2 + O2 → 2H2O, how many grams of water are produced from 5.1 mol of oxygen?arrow_forwardAmmonia (NH3) is an important compound since it is used in large amounts for the manufacture of nitrogenous fertilizers, nylon and many other important compounds. It is manufactured industrially by the catalytic reaction between nitrogen between nitrogen and hydrogen, according to the following equation; N2(g) + H2(g) ⇌ NH3(g) When 0.120 mol nitrogen and 1.20 mol hydrogen are mixed together in a closed vessel, 30% of the nitrogen is converted into ammonia. a. Calculate the moles of nitrogen gas that will be present in the vessel? (only 3 decimal places) b. Calculate the moles of hydrogen gas that will be present in the vessel? (only 3 decimal places c. Calculate the moles of ammonia gas that will be present in the vessel? (only 3 decimal places) d. What is the number of moles of nitrogen gas that has reacted? (only 3 decimal places) Blank 4. Fill in the blank, read surrounding text. mol d. What mass of ammonia can be produced from the limiting reactant? (only 3 decimal placesarrow_forwardGiven the reaction: 4NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (l)When 1.25 mole of ammonia reacts, what will be the total number of moles ofproducts formed?arrow_forward
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning