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Assuming complete combustion, 500.g of pentane (C5H12) reacts with 1.00 kg of oxygen gas. 1. What...
Assuming complete combustion, 500.g of pentane (C5H12) reacts with 1.00 kg of oxygen gas. 1. What is the limiting reagent? 2. What is the theoretical yield of water? 3. If 350. grams of water are produced, what is the percent yield?
Assuming complete combustion, 500.g of pentane (C3H12) reacts with 1.00 kg of oxygen gas. 1. What is the limiting reagent? 2. What is the theoretical yield of water? 3. If 350. grams of water are produced, what is the percent yield? SHOW ALL YOUR WORK FOR FULL CREDIT!
1.Assuming complete combustion, 500. g of pentane (C5H12) reacts with 1.00 kg of oxygen gas. a. What is the limiting reagent? b. What is the theoretical yield of water? c. If 350. grams of water are produced, what is the percent yield? 2. What is the molarity of a solution of HClO3 made from weighing 25.26 g of HClO3 and dissolving it in enough water to make a total volume of 325.0 mL? Calculate the pH of this solution. Is...
Assuming complete combustion, 1.00 kg of pentane (C3H12) reacts with 500 grams of oxygen gas. 1. What is the limiting reagent? 2. What is the theoretical yield of water? 3. If 150. grams of water are produced, what is the percent yield? SHOW ALL YOUR WORK FOR FULL CREDIT!
The hydrocarbon, pentane, C5H12, reacts with oxygen to form carbon dioxide and water. In a 3.00 L container at 25 ºC are placed 0.520 moles of O2 gas and 0.400 moles of solid C5H12. b) How many moles of CO2(g) is produced?
Pentane (C5H12) burns in oxygen to produce carbon dioxide and water via the following reaction: C5H12(g)+8O2(g)) Δ⟶ 5CO2(g)+6H2O(g) Calculate the mass of CO2 that can be produced if the reaction of 36.5 g of pentane and sufficient oxygen has a 65.0 % yield.
A mixture of methane gas, CH4(g), and pentane gas, C5H12(g), has a pressure of 0.5427 atm when placed in a sealed container. The complete combustion of the mixture to carbon dioxide gas, CO2(g), and water vapor, H2O(g), was achieved by adding exactly enough oxygen gas, O2(g), to the container. The pressure of the product mixture in the sealed container is 2.417 atm. Calculate the mole fraction of methane in the initial mixture assuming the temperature and volume remain constant.
The combustion of pentane can be represented by the following equation: __C5H12 (g) + __O2(g) → __CO2(g) + __H2O(g) Balance the equation and answer the next three questions. 1. If 270. g of C5H12 and 970. g O2 react, which reactant is used up first? (enter pentane or oxygen) 2. What is the mass of carbon dioxide produced? (Give your answer to 3 sig figs.) grams 3. What is the mass of water produced?(Give your answer to 3 sig figs.)...
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
What is this question asking? The reaction of 5.0g of pentane (C5H12) with 5.0g of oxygen gas produces 20.4g of CO2. What is the percent yield of this reaction?