. If 6.5 g of zinc reacts with 5.0 g of HCl, according to the following reaction. Zn + 2HCl -> ZnCl2 + H2 a) Which substance is the limiting reactant? b) How many grams of the reactant remain unreacted?
Question
. If 6.5 g of zinc reacts with 5.0 g of HCl, according to the following reaction. Zn + 2HCl -> ZnCl2 + H2 a) Which substance is the limiting reactant? b) How many grams of the reactant remain unreacted?
Solution
To answer these questions, we need to use the concept of stoichiometry, which is the calculation of relative quantities of reactants and products in chemical reactions.
a) To find the limiting reactant, we first need to find the number of moles of each reactant. We can do this using the molar mass of each substance. The molar mass of zinc (Zn) is about 65.38 g/mol and the molar mass of HCl is about 36.46 g/mol.
Number of moles of Zn = 6.5 g / 65.38 g/mol = 0.099 mol Number of moles of HCl = 5.0 g / 36.46 g/mol = 0.137 mol
The stoichiometry of the reaction tells us that 1 mol of Zn reacts with 2 mol of HCl. So, for 0.099 mol of Zn, we need 0.099 x 2 = 0.198 mol of HCl. But we only have 0.137 mol of HCl. Therefore, HCl is the limiting reactant because it will be completely consumed before Zn.
b) To find out how much of the other reactant remains unreacted, we need to calculate how much was used. We know that 1 mol of Zn reacts with 2 mol of HCl, so 0.137 mol of HCl reacts with 0.137/2 = 0.0685 mol of Zn.
The mass of Zn that reacted = 0.0685 mol x 65.38 g/mol = 4.48 g
So, the amount of Zn that remains unreacted = 6.5 g - 4.48 g = 2.02 g.
Similar Questions
To solve this problem, we will follow these steps: a) Determine the limiting reactant: Calculate the moles of each reactant: Moles of Zn: 6.5 g / molar mass of Zn Moles of HCl: 5.0 g / molar mass of HCl Use the stoichiometry of the reaction to determine the moles of product formed from each reactant: Moles of ZnCl2 from Zn: moles of Zn / 1 (from the balanced equation) Moles of ZnCl2 from HCl: moles of HCl / 2 (from the balanced equation) The limiting reactant is the one that produces the least amount of product. In this case, HCl is the limiting reactant because it produces less ZnCl2 compared to Zn. b) Calculate the grams of the reactant that remain unreacted: Calculate the moles of HCl consumed in the reaction. Calculate the moles of HCl remaining by subtracting the moles consumed from the initial moles. Convert the remaining moles of HCl to grams. c) Calculate the grams of hydrogen gas produced: Determine the moles of H2 produced from the moles of HCl consumed. Convert the moles of H2 to grams using the molar mass of hydrogen gas. Given: Molar mass of Zn = 65.38 g/mol Molar mass of HCl = 36.46 g/mol Molar mass of H2 = 2.02 g/mol Let's perform the calculations: a) Limiting reactant: Moles of Zn: 6.5 g / 65.38 g/mol = 0.0994 mol Moles of HCl: 5.0 g / 36.46 g/mol = 0.137 mol Moles of ZnCl2 from Zn: 0.0994 mol Moles of ZnCl2 from HCl: 0.137 mol / 2 = 0.0685 mol HCl is the limiting reactant because it produces less ZnCl2. b) Remaining unreacted HCl: Initial moles of HCl = 0.137 mol Moles of HCl consumed = 0.137 mol - 0.0685 mol = 0.0685 mol Remaining moles of HCl = 0.137 mol - 0.0685 mol = 0.0685 mol Remaining grams of HCl = 0.0685 mol * 36.46 g/mol = 2.50 g c) Grams of hydrogen gas produced: Moles of H2 produced = 0.0685 mol (from the consumed HCl) Grams of H2 produced = 0.0685 mol * 2.02 g/mol = 0.1387 g Therefore: a) HCl is the limiting reactant. b) 2.50 grams of HCl remain unreacted. c) 0.1387 grams of hydrogen gas would be produced.
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