Multiple Choice
For the reaction 3A + 2B + C → 2D, if 5.7 mol of A, 3.2 mol of B, and 2.5 mol of C are mixed, which reactant is the limiting reactant?
3. Chemical Reactions
Stoichiometry
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How many grams of CaCl2 are formed when 15.00 mL of 0.00237 M Ca(OH)2 reacts with excess Cl2 gas according to the reaction: 2 Ca(OH)2(aq) + 2 Cl2(g) → Ca(OCl)2(aq) + CaCl2(s) + 2 H2O(l)?
A
0.00474 g
B
0.00394 g
C
0.00197 g
D
0.00237 g
Verified step by step guidance1
First, identify the balanced chemical equation for the reaction: 2 Ca(OH)2(aq) + 2 Cl2(g) → Ca(OCl)2(aq) + CaCl2(s) + 2 H2O(l). This equation shows the stoichiometry of the reactants and products.
Calculate the number of moles of Ca(OH)2 using the molarity and volume of the solution. Use the formula: \( \text{moles} = \text{molarity} \times \text{volume in liters} \). Convert 15.00 mL to liters by dividing by 1000.
Using the stoichiometry from the balanced equation, determine the moles of CaCl2 produced. According to the equation, 2 moles of Ca(OH)2 produce 1 mole of CaCl2. Therefore, divide the moles of Ca(OH)2 by 2 to find the moles of CaCl2.
Convert the moles of CaCl2 to grams using its molar mass. The molar mass of CaCl2 can be calculated by adding the atomic masses of calcium (Ca) and chlorine (Cl) from the periodic table: \( \text{molar mass of CaCl2} = \text{molar mass of Ca} + 2 \times \text{molar mass of Cl} \).
Finally, multiply the moles of CaCl2 by its molar mass to find the mass in grams. This will give you the mass of CaCl2 formed in the reaction.
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