The diagram below represents the reaction between ammonia and oxygen to produce nitric oxide and water. Use this diagram to calculate the number of moles of nitric oxide that could be produced from 12 moles of ammonia.

For the following unbalanced reaction,

SrS + Co₂(SO₄)₃ → SrSO₄ + Co₂S₃

Determine the mass of Co₂(SO₄)₃ required to completely react with 78.6 g of SrS.

The image below shows the reaction between A (green spheres) and B₂ (orange spheres) to form AB₃.

(i) Identify the limiting reagent in the image, and (ii) calculate the moles of AB₃ formed using 1.0 mol of A and 1.0 mol of B₂.

Alkali metals are highly reactive and react violently with water. To protect them from water, alkali metals are kept in kerosene oil. The reaction of sodium metal with water produces sodium hydroxide and hydrogen gas. Due to the exothermic nature of the reaction and the high flammability of hydrogen gas, flames are produced. Assuming that the reaction is carried out in absence of oxygen gas, determine how much hydrogen gas is produced when a 2.55 g piece of sodium metal reacts with 5.15 g liquid water.

Consider the following reaction:

2CuS(s) + 3O₂(g) → 2CuO(s) + 2SO₂(g)

Initially, the reaction mixture contains 3.0 mol CuS and 4.0 mol O₂. How many moles of the excess reactant remains after the reaction has occurred completely?

Hematite is a common iron oxide compound with the formula Fe₂O₃ and is widely found in rocks and soils. The iron can then be extracted from the Hematite by the following set of reactions: 

3 Fe₂O₃ + CO → 2 Fe₃O₄ + CO₂

Fe₃O₄ + CO → 3 FeO + CO₂

FeO + CO → Fe + CO₂

Suppose that the first and second reaction is carried out with an 85.6 % yield. If the third reaction is carried out with a 95.6 % yield, what mass of iron can be obtained from 5.00 kg of hematite? 

The reaction of ammonia with carbon dioxide produces urea CH₄N₂O, a common fertilizer according to the following equation (note: the reaction is unbalanced):

NH₃(aq) + CO₂(aq) → CH₄N₂O(aq) + H₂O(l)

A chemist uses 32.5 mg of NH₃ with 89.6 mg of CO₂ to produce 55.7 mg of urea in the industrial urea synthesis. Answer the following questions:

(a) What is the limiting reactant?

(b) What is the theoretical yield of urea?

(c) What is the percent yield for the reaction?

The compound 1-hexene (C₆H₁₂) reacts with water to form 2-hexanol (C₆H₁₄O): C₆H₁₂ + H₂O → C₆H₁₄O. In an experiment, 10.0 mL of 1-hexene (d = 0.673 g/mL) is reacted with 6.0 mL of water (d = 1.00 g/mL), resulting in 7.8 mL of 2-hexanol (d = 0.810 g/mL). Calculate the percent yield of the reaction.

At 25°C, 100 mL of isopropyl alcohol (C₃H₈O) was mixed with 42.9 mL of water to create a solution. At the same temperature, the densities of isopropyl alcohol and water are 0.781 g/mL and 1.00 g/mL, respectively. What is the concentration of this solution in percent by mass?

Sodium can be reacted with oxygen at 130–200°C to produce sodium oxide (Na₂O, white powder) and sodium peroxide (Na₂O₂, yellow solid). Sodium oxide can further absorb oxygen to produce sodium peroxide. A piece of sodium metal was reacted with oxygen and produced a mixture of 0.496 g of white and yellow solid. The mixture was further exposed to oxygen until the final product is pure yellow solid with a mass of 0.525 g. Calculate the mass percentage of sodium oxide in the initial mixture.  

Gallium(III) iodide is composed of 84.52% w/w iodine. How many grams of iodine are present in 153.7 g of gallium(III) iodide?

Match each compound with the correct functional group classification. 

Note: Order for multiple choice answers is from left to right and top to bottom

a) Alkene                 b) Alkyne                 c) Alkyl Halide                d) Alcohol

e) Carboxylic Acid    f) Ether                    g) Ester                          h) Aldehyde

i) Ketone                   j) Amine

Identify which of the other compounds exhibit a sour odor like Acetic acid