What is stoichiometry and why is it used in chemistry?

What is stoichiometry and why is it used in chemistry?

1. Stoichiometry is a study of quantitative composition of substances involved in the chemical reactions.
2. A balanced chemical equation can be used to calculate number of moles, number of particles and mass or volume of a reactant or product.
3. By using the information obtained from a balanced chemical equation, it is possible to calculate the quantities of reactants used or the quantities of products formed in the reaction.
4. Generally, the steps involved in the stoichiometric calculations are as follows.
   (1) Write down the balanced equation of the reaction.
   (2) Gather information from the question. If necessary, convert the given unit to the number of moles.
   (3) Based on the equation, compare the ratio of moles of the related substances.
   (4) Calculate the answer proportionately. Then, convert the answer to the required unit.

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Stoichiometry Problems with Answers

1. How many moles of potassium are needed to react with 0.5 mole of bromine gas?
2K(s) + Br₂(g) ⟶ 2KBr(s)
Solution:

2. Ethene gas burns in excessive oxygen according to the following equation.
C₂H₄(g) + 3O₂(g)  ⟶  2CO₂(g) + 2H₂O(l)
Find the volume of carbon dioxide released at STP if 42 g of ethene is burnt completely. [Relative atomic mass: H, 1; C, 12. Molar volume: 22.4 dm³ mol^-1 at STP]
Solution:

3. What is the mass of zinc needed to produce 2.4 dm³ of hydrogen gas at room conditions?
Zn(s) + 2HNO₃(aq) ⟶  Zn(NO₃)₂(aq) + H₂(g)
[Relative atomic mass: Zn, 65. Molar volume: 24 dm³ mol^-1 at room conditions]
Solution:

4. Aluminium reacts with copper(II) oxide to produce aluminium oxide and copper. If 2.0 g of excess aluminium is reacted with 0.06 mole of copper(II) oxide, find the mass of aluminium left after the reaction.
[Relative atomic mass: Al, 27]
Solution:

5. Excess sodium chloride is added to 50.0 cm³ of silver nitrate solution. 2.87 g of silver chloride is precipitated. Calculate the concentration of the silver nitrate solution in mol dm^-3.
[Relative atomic mass: Cl, 35.5; Ag, 108]
Solution:

6. In the preparation of copper(II) sulphate, a student added 4.0 g of copper(II) oxide to 1.25 mol dm^-3 sulphuric acid. Calculate the volume of the acid needed to react completely with the copper(II) oxide. [Relative atomic mass: O, 16; Cu, 64]
Solution:

7. Excess aluminium powder is added to 300 cm³ of 2.0 mol dm^-3 hydrochloric acid. The mixture is then warmed to speed up the reaction. Calculate the mass of the salt formed. [Relative atomic mass: Al, 27; Cl, 35.5]
Solution:

8. 150 cm³ of 1.0 mol dm^-3 ammonia solution is completely neutralised with phosphoric acid using a titration method. Calculate the mass of ammonium phosphate formed. [Relative atomic mass: H, 1; N, 14; O, 16; P, 31]
Solution:

9. 6.20 g of copper(II) carbonate is added to 100 cm³ of 14.6 g dm^-3 hydrochloric acid. Calculate the mass of copper(II) chloride produced. [Relative atomic mass: H, 1; C, 12; O, 16; Cl, 35.5; Cu, 64]
Solution: