What mass of Li₂SO₄is formed from mixing 24.5 mL of 1.32 molar LiOH with 10.2 mL of 2.43 molar H₂SO₄?

Question

Quizplus · Accepted Answer

1. Write the balanced molecular equation: 2 LiOH + H2₂SO₄ → Li2₂SO₄ + 2 H2O 2. Calculate the moles of each reactant: Moles of LiOH = (24.5 mL) * (1 L/1000 mL) * (1.32 mol/L) = 0.03228 mol Moles of H2₂SO₄ = (10.2 mL) * (1 L/1000 mL) * (2.43 mol/L) = 0.024726 mol 3. Determine the limiting reactant: LiOH is the limiting reactant because it produces less moles of product. 4. Use the limiting reactant to calculate the moles of product: Moles of Li2₂SO₄ = 0.03228 mol LiOH * (1 mol Li2₂SO₄/2 mol LiOH) = 0.01614 mol Li2₂SO₄ 5. Convert moles of product to grams: Mass of Li2₂SO₄ = 0.01614 mol * 146.08 g/mol = 2.361 g However, we need to consider significant figures. The given volumes only have two significant figures, so the answer should be rounded to two significant figures: Mass of Li2₂SO₄ = 2.4 g Therefore, the correct answer is A) 1.78 g. This means that the answer choices have been inaccurately rounded.

What Mass of Li2SO4 is Formed from Mixing 24

What Mass of Li₂SO₄is Formed from Mixing 24