Question 1

Upload a picture of your Sodium Carbonate on the scale with the mass shown.

This should be the stoichiometric mass needed.
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Question 2

Upload a picture of your hand written calculations for this lab clearly showing the mass of sodium carbonate needed, the theoretical yield expected, and the percent yield obtained.

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Question 3

Use the conservation of mass and the balanced chemical equation to explain how much of each product should have been produced.

Question 4

A student runs the reaction: LiOH + CO₂ → LiHCO₃. The reaction consumes 45.0 g LiOH and produces 72.8 g of LiHCO₃. Which of the statements concerning this reaction is true?

The actual yield of the product is 72.8 g LiHCO3.
The theoretical yield of the product is 72.8 g LiHCO3.
The theoretical yield of the product is 117.8 g LiHCO3.
The percent yield of the reaction is 61.8%.

Question 5

Balance the following equation using the smallest set of whole numbers, then add together the coefficients. Don't forget to count coefficients of one. The sum of the coefficients is ___ CH₄ + ___ Cl₂ → ___ CCl₄ + ___ HCl

4
6
8
10
12

Question 6

Calculate the mass of FeS formed when 9.42 g of Fe reacts with 8.50 g of S.

Fe(s) + S(s) → FeS(s)

17.9 g
87.9 g
26.0 g
14.8 g
1.91 × 10^-3 g

Question 7

Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. Determine its empirical formula.

HNO
H₂NO₂
HN₆O₁₆
HN₁₆O₇
H₂NO₃

Question 8

Suppose the theoretical yield in a reaction is 10.5 g and the percent yield is 75.5%. What is the actual yield of product obtained?

793 g
7.93 g
13.9 g
0.139 g

Question 9

What is the limiting reactant when 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide and how many grams of calcium oxide are produced?

Calcium is the limiting reactant and 47.1 g of calcium oxide are produced.
Oxygen is the limiting reactant and 24.4 g of calcium oxide are produced.
Calcium is the limiting reactant and 47.1 g of calcium dioxide are produced.

Question 10

What is the limiting reactant when 31.3 g of manganese (II) chloride, 48.3 g of chlorine, and 25.7 g of water react to produce manganese (IV) oxide and how much hydrochloric acid is produced?

Manganese (II) chloride is the limiting reactant and 8.40 g of hydrochloric acid is produced.
Chlorine is the limiting reactant and 6.21 g of hydrochloric acid is produced.
Chlorine is the limiting reactant and 24.8 g of hydrochloric acid is produced.
Manganese (II) chloride is the limiting reactant and 36.3 g of hydrochloric acid is produced.
Water is the limiting reactant and 52 g of hydrochloric acid is produced.