How many grams of each product result from the following reactions, and how many

Question

How many grams of each product result from the following reactions, and how many grams of which reactant is left over?

Part A

( 1.4 g NaCl)+( 3.1 g AgNO3)(xgAgCl)+(ygNaNO3)

AgNO3 = limiting reactant

Part B

Enter your answers numerically separated by commas. Express your answer using two significant figures.

mNaCl,mAgCl,mNaNO3 = ?

Note: I got .35, 2.6, 1.5 - apparently 2.6 is correct, but .35 and 1.5 are incorrect but theyre very close. It seems to be a significant figures rule but I cant figure out what Im doing wrong ive calculated it several times

Explanation / Answer

( 1.4 g NaCl)+( 3.1 g AgNO3)(xgAgCl)+(ygNaNO3)

As per balanced equation one mole of NaCl will react with one mole of AgNO3 to give one mole of each product

The mole of NaCl present = Mass / Molar mass = 1.4 / 58.5 = 0.0239

Moles of AgNO3 = Mass / Molar mass = 3.1 / 169.87 = 0.0182

so limiting reagent is AgNO3

Moles of NaCl left after reaction = 0.0239 - 0.0182 = 0.0057

Mass of NaCl left = Moles X molar mass = 0.0057 X 58.5 = 0.333

Moles of each product formed = 0.0182

Mass of AgCl formed = Moles X molar mass = 0.0182 X 143.32 = 2.61 grams

Mass of NaNO3 = Moles X molar mass = 0.0182 X 85 = 1.55 grams

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