15.00g of Aluminium Sulphide and 10.00g water react until the limiting reagent is used up. Here is the balance equation for the reaction.
Al₂S₃ + 6H₂O → Al(OH)₃ + 3H₂S

a) Which is the limiting reagents?
b) What is the maximum mass of H₂S which can be formed from these reagents?
c) How much excess reagents remains after the reaction is complete?

If there is 35.0 grams of C₆H₁₀ and 45.0 grams of O₂, how many grams of the excess reagent will remain after the reaction ceases?
2 C₆H₁₀ + 17 O₂ → 12 CO₂ + 10 H₂O

a) What mass of AL₂O₃ can be produced from the reaction of 10.00g of AL and 19.0g of O₃?
b) How much of the excess reagent remains unreacted?

Based on the balanced equation
C₄H₈ + 6O₂ → 4 CO₂ + 4 H₂O

Calculate the number of excess reagent units remaining when 28 C₄H₈ molecules and 228 O₂ molecules react.

Determine the limiting reagent of this reaction.
Na₂B₄O₇ + H₂SO₄ + 5H₂O → 4H₃BO₃ + Na₂SO₄
There are 5.00g of each reactant.

How much O₂ could be produced from 2.45g of KO₂ and 4.44g of CO₂?
4KO₂ + 2CO₂ → 2K₂CO₃ + 3O₂

a) What mass of hydrogen peroxide should result when 1.45g of barium peroxide is treated with 25.5mL of hydrochloric acid solution containing 0.0277g of HCL per mL?
b) How much of the excess reactant is left?

BaO_2(S)+ 2HCL_(aq) → H₂O_(2aq) + BaCL_(2aq)

A 2.00g sample 0f ammonia is mixed with 4.00g of Oxygen. Which is the limiting reactant and how much excess reactant remain after the reaction has stopped?
Balanced equation for the reaction:
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(s)

90.0 of FeCL₃ react with 52.0g of H₂
i. What is the limiting reactant?
ii. What is the mass of HCL produced?
iii. What mass of excess reactant remain after the reaction?

If 120.0g of propane, C₃H₈ is burned in excess oxygen how many of water are formed.

How many moles of nitrogen are there in a 7.45 mole sample of ammonium phosphate?

How many grams of carbon dioxide are there in a container with a volume of 4.5L at STP?

A sample contains 27.2g of calcium Oxide. How many moles of calcium Oxide are there in the sample?

Take the reaction
NH₃ + O₂ → NO + H₂

In an experiment 325g of NH3 are allowed to read with 3.5g of O₂ a) Which reactant is the limiting reagent?
b) How many gram of NO are formed?
c) How much of the excess reactant remain after the reactant?

If 4.95g 0f ethylene (C₂H₄) are combusted with 3.25g of Oxygen
a) What is the limiting reagent?
b) How many gram of CO₂ are formed?

Consider the reaction of C₆H₂ + Br₂ → C₆H₅Br + HBr
a) What is the liming reagent if 42.1g of C₆H₆ react with 73.0g of Br₂?

A reaction container holds 5.77g of P₄ and 5.77g of O₂. The following reaction occur

P₄ + O₂ → P₄O₆

If there were enough Oxygen were available, then the P₄O₆ reacts further;
P₄O₆ + O₂ → P₄O₁₀

Calculate;
i. Mode of P₄O₁₀ produced
ii. Mass of P₄O₁₀ produced.

a) Give the meaning of the following terms
i/ Excess reagents
ii/ limiting reagents
b) How to identify the limiting and excess reagent in stoichiometry?

6 mole of nitrogen reacted with 8moles of hydrogen to produce ammonia gas at stp.
a) Identify
i/ limiting reagent
ii/ Excess reagent
b) Calculate the volume of ammonia gas produced at stp by Haber process.

a) Give the meaning of stoichiometry.
b) Outline procedures to be considered when dealing with stoichiometric calculation problems.
c) Mention Procedures to be considered on dealing with excess and limiting reagents problems.

Calculate the volume of oxygen gas product at STP when 12.25g of potassium chlorate are decomposed by heating according to the equation below.

2KCLO_3(S) heat→ 2KCL_(S) + 30_2(S)

Ammonium chloride reacts with calcium hydroxide as shown in the following equation.

NH_4(aq) + Ca(OH)_2(aq) → NH₃ + CaCl_2(aq) + H_2(l)

Calculate the mass of ammonium chloride NH4CI that will read completely with 14.8g of calcium hydroxide.

Sodium sulphate react with barium nitrate as shown in the equation below.

Na₂SO_4(aq) + Ba (NO3)_2(aq)→BaSO4_s + 2NaNO_2(aq)

How many moles of barium Sulphate are produced when 80.5g of Sodium Sulphate react completely with barium nitrate?

4.90g of copper (II) Oxide yielded 3.92g of copper when reduced by hydrogen gas.
Calculate the mass of copper (II) oxide required to yield 4g of copper. (Cu=64, O=16)

The decomposition of Pb(NO₃)₂ is as shown below.

Pb(NO₃)_2(S)→2PbO_(S) + 4NO_2(g) + O_2(g)

If 0.01 mole of the nitrate was used, what would be the maximum volume of oxygen gas collected at room temperature and pressure?
(molar gas volume at rtp = 24.0 cm³3)

What mass of anhydrous Sodium Carbonate would be required to completely react with 20cm³ of 0.4M Sulphuric acid solution.
(Na = 23, 0 = 16, C = 12, H = 1)

1.63g of Zinc metal was added to excess Silver Nitrate Solution. The mass of silver formed was 5.40g.
(Zn = 65, Ag = 108)
What is the equation for the displacement reaction?
Show the working.

100 cm³ of 1M NaOH was mixed with 100 cm³ of 0.1M HCI.
After the reaction.
a. Which ions were in excess and by how much?
b. Find the concentration of the excess ions.

Lead nitrate decomposes on heating as shown in the equation below.
Pb (NO₃)₂ heat → 2PbO_(S) + 4N0_2(S) + O_2(g)

112dm³ of oxygen gas were collected at STP when a sample of lead nitrate was completely decomposed by heating. Calculate;
a. The mass of the lead nitrate sample.
b. The mass of lead (II) oxide produced.
c. The volume of nitrogen dioxide gas produced at STP.
(Pb = 207, Na =14, 0 = 16; molar volume of a gas at STP = 22.4 dm³)

The equation below shows the reaction the reaction between heated copper (II) oxide and ammonia gas.
3CuO_(g) + 2 NH_3(g) → 3Cu_(S) + N_2(g) + 3H₂O_(l)

If 20g of copper (II) oxide reacted with ammonia gas at STP.
Calculate;
a. The number of moles of copper (II) oxide used.
b. The volume of ammonia gas used.
c. The mass of copper formed.
(Cu = 64, 0 = 16, N = 14, H = 1. Molar volume of a gas at STP = 22.4 dm³)