Question

If 73.5 g of liquid Br2 and 330 mL of 1.18 M aqueous NaI are reacted stoichiometrically according to the balanced equation, how many grams of liquid Br2 remain? Round your answer to 3 significant figures.

2NaI(aq) + Br2(l) → 2NaBr(aq) + I2(s)
mols NaI = 0.330 x 1.18 = 0.389
How much Br2 will it use? Look at the coefficients in the balanced equation. It will need half of that; therefore, 0.389/2 = ? mols Br2 use. How many grams is that? g = moles Br2 used x molar mass.
75.3 g initially - g used = g remaining. Check all of my numbers. I rounded here and there.

Related Questions

If 0.670mol of liquid Br2 and 460mL of 1.72M aqueous NaI are reacted stoichiometrically according to... If 0.870 mol of liquid Br2 and 720 mL of 0.958 M aqueous NaI are reacted stoichiometrically accordi... If 890 mL of 0.236 M aqueous NaI and 0.560 mol of liquid Br2 are reacted stoichiometrically accordi... If 890 mL of 0.236 M aqueous NaI and 0.560 mol of liquid Br2 are reacted stoichiometrically accordin...