Using the initial quantities for each reactant and the final quantity of nitrogen dioxide produced, determine...
Using the initial quantities for each reactant and the final quantity of nitrogen dioxide produced, determine the limiting reactant, theoretical yield and the percent yield?
54.8 g ammonia
29.8 g oxygen
12.4 nitrogen dioxide
4NH3(g) + 5O2(g) = 4NO(g) + 6H2O(g)
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Using the initial quantities for each reactant and the final
quantity of nitrogen dioxide produced, determine...
1. Based on the initial quantities given, which is the limiting reactant? How many grams of...
1. Based on the initial quantities given, which is the limiting reactant? How many grams of each product will be produced based on this? 12.3 g NaOH 11.9 g HCl NaOH(aq) + HCl(aq) = H2O(l) + NaCl(aq) 2. Using the initial quantities for each reactant and the final quantity of hydrochloric acid produced, determine the limiting reactant, the theoretical yield and the percent yield. 34.67 g hydrogen 21.88 g chlorine 12.34 g hydrochloric acid H2(g) + Cl2(g) ® 2HCl(g)
1) Ammonia, NH3, reacts with molecular oxygen, O2, to formnitric oxide, NO, and water:4NH3(g)...
1) Ammonia, NH3, reacts with molecular oxygen, O2, to form
nitric oxide, NO, and water:4NH3(g) + 5O2(g) = 4NO (g) +6H2O(l)A. What is the limiting reactant and what is the theoretical
yield of NO?B. What is the theoretical yield of H2O?C. How many grams of excess reagent will be left over?D. If the actual yield of NO had been 91 g, what would be the
percent yield of the reaction
For each of the following reactions, 32.0 g of each reactant is present initially. A. 1....
For each of the following reactions, 32.0 g of each reactant is present initially. A. 1. Determine the limiting reactant. 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) 2. Calculate the grams of product in parentheses that would be produced. (H2O) B. For each of the following reactions, 32.0 g of each reactant is present initially. 1. Determine the limiting reactant. CS2(g)+3O2(g)→CO2(g)+2SO2(g) 2. Calculate the grams of product in parentheses that would be produced. (CO2)
2. a. Nitrogen dioxide and hydrogen are reacted in the gas phase, in the presence of...
2. a. Nitrogen dioxide and hydrogen are reacted in the gas phase, in the presence of a catalyst, to produce ammonia and water; write a balanced equation for this reaction. (2 pts) b. If 73.2 g of nitrogen dioxide and 10.6 g of hydrogen are mixed together and react to form ammonia, identify the limiting reactant and calculate the theoretical yield (in grams) of ammonia produced. (6 pts) c. 12.9 g of ammonia is actually produced in this reaction; based...
Limiting Reactant, Theoretical Yield and Percent Yield 2. Pentane combusts with en to form carbon dioxide...
Limiting Reactant, Theoretical Yield and Percent Yield 2. Pentane combusts with en to form carbon dioxide and water by the following reaction: CsHız(1) + 8 O2(g) → 5 CO2(g) + 6H2O(g) a. If 8.00 g of pentane is mixed with 10.0 g of oxy compare it to either of the products). he is mixed with 10.0 g of oxygen, which is the limiting reactant? (Hint: b. What is the theoretical yield (in grams) of carbon dioxide and water for this...
--xal Yield and Percent Yield combusts with oxygen to form carbon dioxide and water by the...
--xal Yield and Percent Yield combusts with oxygen to form carbon dioxide and water by the following reaction: pentane combud CsHız(l) + 8 O2(g) → 5 CO2(g) + 6 H2O(g) a. If 8.00 g of pentane is mixed with 10.0 g of oxygen, which is the limiting reactant? (Hint: compare it to either of the products). b. What is the theoretical yield (in grams) of carbon dioxide and water for this reaction? Hydrogen reacts with nitrogen to form ammonia by...
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in...
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H2O that can produced by combining 67.5 g of each reactant? 4NH3(g)+5O2(g)-------- >4NO(g)+6H2O(g)
1. Moles of Reactant to Mass of Reactant: Identify the iodide ions and ozone in the...
1. Moles of Reactant to Mass of Reactant: Identify the iodide ions and ozone in the balanced chemical equation. Use mole ratio, then convert to grams. A method used by the EPA for determining the ozone concentration in the air is to pass an air sample through a bubbler containing iodide ions. The iodide ions remove the ozone according to the following reaction: O3(g) + 2 I-(aq) + H2O(l) → O2(g) + I2(aq) + 2 OH-(aq) How many grams of ozone...
Determine the limiting reactant and calculate the number of grams of nitrogen dioxide, NO, that can...
Determine the limiting reactant and calculate the number of grams of nitrogen dioxide, NO, that can be formed when 105 g of nitrogen, N, reacts with 98.5 g of oxygen, N.(9) + 2 0,(9) - 2 NO (9)
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in...
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H2OH2O that can be produced by combining 86.7 g86.7 g of each reactant? 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(g)
1) Ammonia, NH3, reacts with molecular oxygen, O2, to form
nitric oxide, NO, and water:4NH3(g) + 5O2(g) = 4NO (g) +6H2O(l)A. What is the limiting reactant and what is the theoretical
yield of NO?B. What is the theoretical yield of H2O?C. How many grams of excess reagent will be left over?D. If the actual yield of NO had been 91 g, what would be the
percent yield of the reaction
2. a. Nitrogen dioxide and hydrogen are reacted in the gas phase, in the presence of a catalyst, to produce ammonia and water; write a balanced equation for this reaction. (2 pts) b. If 73.2 g of nitrogen dioxide and 10.6 g of hydrogen are mixed together and react to form ammonia, identify the limiting reactant and calculate the theoretical yield (in grams) of ammonia produced. (6 pts) c. 12.9 g of ammonia is actually produced in this reaction; based...
Limiting Reactant, Theoretical Yield and Percent Yield 2. Pentane combusts with en to form carbon dioxide and water by the following reaction: CsHız(1) + 8 O2(g) → 5 CO2(g) + 6H2O(g) a. If 8.00 g of pentane is mixed with 10.0 g of oxy compare it to either of the products). he is mixed with 10.0 g of oxygen, which is the limiting reactant? (Hint: b. What is the theoretical yield (in grams) of carbon dioxide and water for this...
--xal Yield and Percent Yield combusts with oxygen to form carbon dioxide and water by the following reaction: pentane combud CsHız(l) + 8 O2(g) → 5 CO2(g) + 6 H2O(g) a. If 8.00 g of pentane is mixed with 10.0 g of oxygen, which is the limiting reactant? (Hint: compare it to either of the products). b. What is the theoretical yield (in grams) of carbon dioxide and water for this reaction? Hydrogen reacts with nitrogen to form ammonia by...
Determine the limiting reactant and calculate the number of grams of nitrogen dioxide, NO, that can be formed when 105 g of nitrogen, N, reacts with 98.5 g of oxygen, N.(9) + 2 0,(9) - 2 NO (9)
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