Day 1  Day 2  Day 3  Day 4  Day 5  Day 6

Day 1

Question 1

Aqueous iron(III) chloride, FeCl3, reacts with aqueous potassium iodide, KI.

vFeCl3​​ + wKI​​ ​​ xFeCl2​​ + yKCl + I2

Which statements are correct?

• In the balanced equation, v, w, x and y have the same value.

• Potassium iodide is an oxidising agent.

• A dark brown solution is produced in the reaction.

• 1 and 2

• 1 and 3

• 2 only

• 2 and 3

Question 2

The relative atomic mass, Ar, of an element is the average mass of the isotopes of that element compared to another particle.

Which particle is used for this comparison?

• A proton

• An atom if​​ 12C

• An atom of​​ 40Ca

• An atom of​​ 1H

Day 2

Question 1

The equation for the combustion of methane is shown.

CH4​​ + 2O2​​ ​​ CO2​​ + 2H2O

Which mass of methane produces 36g of water?

• 16​​ g

• 18​​ g

• 32​​ g

• 64​​ g

Question 2

Calcium carbonate, CaCO3, reacts with dilute hydrochloric acid to produce carbon dioxide.

The equation for the reaction is shown. The relative formula​​ mass of calcium carbonate is 100.

CaCO3​​ + 2HCl​​ ​​ CaCl2​​ + H2O + CO2

10g of calcium carbonate is reacted with excess of dilute hydrochloric acid.

Which mass of carbon dioxide is produced?

• 2.2 g

• 2.8 g

• 4.4 g

• 44 g

Day 3

Question 1

The equation for the reaction between sodium carbonate and excess dilute hydrochloric acid shown.

Na2CO3​​ + 2HCl​​ ​​ 2NaCl + H2O + CO2

When 26.5 g of sodium carbonate reacts with excess dilute hydrochloric acid, what is the maximum volume of carbon dioxide produced?

• 6 dm3

• 12 dm3

• 18dm3

• 24dm3

Question 2

The equation shows the reaction between magnesium and sulfuric acid.

[Ar: H, 1; O, 16; Mg, 24; S, 32]

Mg + H2SO4​​ ​​ MgSO4​​ + H2

In this reaction, which mass of magnesium sulfate is formed when 6 g of magnesium react with excess sulfuric acid?

• 8 g

• 24 g

• 30 g

• 60 g

Day 4

Question 1

A compound contains 1.10 mol of K, 0.55 mol of C, and 1.65 mol of O. What is the empirical formula of this compound?

Question 2

An organic compound contains carbon, hydrogen, and oxygen. If elemental analysis reveals 38.71% carbon and 9.67% hydrogen, which is its empirical formula?

• CH3O

• CH2O

• CHO

• CH4O

Day 5

Question 1

Magnesium reacts with steam.

Mg + H2O​​ ​​ MgO + H2

When 2.43g of magnesium reacts with an excess of steam, the products are 4.03 g of magnesium oxide and 0.20 g of hydrogen.

What is produced when 7.29 g of magnesium is reacted with an excess of steam?

• 1.34 g of magnesium oxide and 0.07 g of hydrogen.

• 4.03 g of magnesium oxide and 0.20 g of hydrogen.

• 8.06 g of magnesium oxide and 0.40 g of hydrogen.

• 12.09 g of magnesium oxide and 0.60 g of hydrogen.

Day 6

Question 1

The equation for the thermal decomposition of sodium hydrogencarbonate is shown.

2NaHCO3​​ ​​ Na2CO3​​ + H2O + CO2

The Mr​​ of sodium hydrogencarbonate, NaHCO3, is 84.

The Mr​​ of sodium carbonate, Na2CO3, is 106.

In an experiment, 2.1 g of sodium hydrogencarbonate is heated but not all of it decomposes. All of the carbon dioxide is collected and measured at room temperature and pressure. The total volume of carbon dioxide produces id 0.21dm3.

The volume of 1 mole of gas at room temperature and pressure is 24dm3.

Which statement is correct?

• The mass of sodium carbonate produced is 0.93 g.

• The mass of sodium carbonate produced is 1.33 g.

• The percentage yield of carbon dioxide is 10%.

• The percentage yield of carbon dioxide is 35%.