09 - (d) How many moles of the excess reactant remain...

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Practice 1: Consider the reaction: 2Sb (s) + 3I 2 (s) 2SbI 3 (s) Determine the limiting reactant and the theoretical yield when (a) 1.20 mol of Sb and 2.40 mol of I 2 are mixed. (b) 1.20 grams of Sb and 2.40 grams of I 2 are mixed. What mass of excess reactant is left when the reaction is complete? Practice 2: Iron reacts with chlorine gas to form Iron (III) chloride. If you start with 2.75 mol of Iron and 3.50 mol of Chlorine, (a) Write a balanced equation for the reaction (b) What is the limiting reagent? (c) What is the theoretical yield of Iron (III) chloride in grams? (d) How many moles of excess reactant remain unreacted? (e) How many grams of excess reactant remain unreacted?
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Practice 3: A gaseous mixture containing 13.0 grams of hydrogen gas and 1280.00 grams of Bromine react to form Hydrogen bromide gas. (a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) What is the theoretical yield of hydrogen bromide in grams?
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Unformatted text preview: (d) How many moles of the excess reactant remain unreacted? (e) How many grams of the excess reactant remain unreacted? Practice 4: A 199.8 gram sample of Aluminum is reacted with 174.72 liters of gaseous Oxygen at STP to produce Aluminum oxide. (a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) What is the theoretical yield of Aluminum oxide in grams? (d) How many moles of the excess reactant remain unreacted? (e) How many grams of the excess reactant remain unreacted? Practice 5: 4.21 X 10 22 molecules of Hydrogen gas react with 3.01 X 10 22 molecules of oxygen to produce water. (a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) What is the theoretical yield of water in grams? (d) How many moles of excess reactant remain unreacted? (e) How many grams of excess reactant remain unreacted?...
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09 - (d) How many moles of the excess reactant remain...

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