Iron reacts with excess Sulphuric acid to give Iron II sulphate. The equation for the reaction is Fe s + H 2 SO 4 aq → FeSO 4 aq + H 2 g . 5 g of Iron gives 13 . 6 g of Iron II sulphate. Using excess acid, how much Iron II sulphate can be obtained from 10 g of Iron.

Fe s + H 2 SO 4 aq → FeSO 4 aq + H 2 g Atomic mass of Iron is 56 . Given that 5 g of Iron gives 13 . 6 g of Iron sulphate. Therefore, 10 g of Iron would give, = 10 × 13 . 6 5 = 27 . 2 g of Iron sulphate.

Iron reacts with excess Sulphuric acid to give Iron II sulphate. The equation for the reaction is Fe s + H 2 SO 4 aq → FeSO 4 aq + H 2 g . 5 g of Iron gives 13 . 6 g of Iron II sulphate. Using excess acid, how much Iron II sulphate can be obtained from 1 g of Iron?

Fe s + H 2 SO 4 aq → FeSO 4 aq + H 2 g Atomic mass of Iron is 56 . Given that, 5 g of Iron gives 13 . 6 g of Iron sulphate. Therefore, 1 g of Iron gives = 1 × 13 . 6 5 = 2 . 72 g of Iron sulphate.

Iron reacts with excess Sulphuric acid to give Iron II sulphate. The equation for the reaction is Fe s + H 2 SO 4 aq → FeSO 4 aq + H 2 g . 5 g of Iron gives 13 . 6 g of Iron II sulphate. How much Iron will be needed to make 136 g of Iron II sulphate?

Fe s + H 2 SO 4 aq → FeSO 4 aq + H 2 g Atomic mass of Iron is 56 . Given that, 5 g of Iron gives 13 . 6 g of Iron sulphate. Therefore, 136 g of Iron sulphate would be obtained from = 5 × 136 13 . 6 = 50 g of Iron.

Iron reacts with excess Sulphuric acid to give Iron II sulphate. The equation for the reaction is Fe s + H 2 SO 4 aq → FeSO 4 aq + H 2 g . 5 g of Iron gives 13 . 6 g of Iron II sulphate. A 10 g of sample of impure Iron II sulphate contains 8 g of iron II sulphate. Calculate the percentage purity of Iron II sulphate.

A pure substance has nothing else mixed with it. But substances always contain unwanted impurities. A 10 g of iron sulphate contains 8 g of pure iron sulphate. Hence, its percentage of purity is: % purity of substance = mass of pure substance in it total mass × 100 % = 8 10 × 100 % = 80 %

HARD

Upper Secondary: IGCSE

IMPORTANT

Earn 100

Calculate the relative formula mass for the ionic compound hydrated Iron $(II)$ sulphate, ${FeSO}_{4} . 7 H_{2} O$ .

Important Questions on Reacting Masses, and Chemical Equations

HARD

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 5 - Reacting Masses, and Chemical Equations>Checkup on Chapter 5>Q 12

Iron reacts with excess Sulphuric acid to give Iron $(II)$ sulphate. The equation for the reaction is $Fe (s) + H_{2} {SO}_{4} (aq) \to {FeSO}_{4} (aq) + H_{2} (g)$ . $5 g$ of Iron gives $13.6 g$ of Iron $(II)$ sulphate.

Using excess acid, how much Iron $(II)$ sulphate can be obtained from $10 g$ of Iron.

HARD

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 5 - Reacting Masses, and Chemical Equations>Checkup on Chapter 5>Q 12

Using excess acid, how much Iron $(II)$ sulphate can be obtained from $1 g$ of Iron?

HARD

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 5 - Reacting Masses, and Chemical Equations>Checkup on Chapter 5>Q 12

Iron reacts with excess Sulphuric acid to give Iron $(II)$ sulphate. The equation for the reaction is $Fe (s) + H_{2} {SO}_{4} (aq) \to {FeSO}_{4} (aq) + H_{2} (g) . 5 g$ of Iron gives $13.6 g$ of Iron $(II)$ sulphate.

How much Iron will be needed to make $136 g$ of Iron $(II)$ sulphate?

HARD

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 5 - Reacting Masses, and Chemical Equations>Checkup on Chapter 5>Q 12

A $10 g$ of sample of impure Iron $(II)$ sulphate contains $8 g$ of iron $(II)$ sulphate. Calculate the percentage purity of Iron $(II)$ sulphate.

HARD

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 5 - Reacting Masses, and Chemical Equations>Checkup on Chapter 5>Q 13

Aluminium is extracted from the ore Bauxite, which is impure Aluminium oxide. $1 tonne (1000 kg)$ of the ore was found to have this composition:

Aluminium oxide $(825 kg)$ , Iron $(III)$ oxide $(100 kg)$ and sand $(75 kg)$

What percentage of this ore has impurities?

HARD

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 5 - Reacting Masses, and Chemical Equations>Checkup on Chapter 5>Q 13

Aluminium is extracted from the ore Bauxite, which is impure Aluminium oxide.

1 tonne (1000 kg)

of the ore was found to have this composition:

Aluminium oxide $(825 kg)$ , Iron $(III)$ oxide $(100 kg)$ and sand $(75 kg)$ .

$1 tonne$ of ore gives $437 kg$ of Aluminium. How much aluminium will be obtained from $5 tonnes$ of the ore?

HARD

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 5 - Reacting Masses, and Chemical Equations>Checkup on Chapter 5>Q 13

Aluminium is extracted from the ore Bauxite, which is impure Aluminium oxide.

1 tonne (1000 kg)

of the ore was found to have this composition:

Aluminium oxide $(825 kg)$ , Iron $(III)$ oxide $(100 kg)$ and sand $(75 kg)$

$1 tonne$ of ore gives $437 kg$ of Aluminium. What mass of sand is in this $5 tonnes$ ?

HARD

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 5 - Reacting Masses, and Chemical Equations>Checkup on Chapter 5>Q 13

Aluminium is extracted from the ore Bauxite, which is impure Aluminium oxide.

1 tonne (1000 kg)

of the ore was found to have this composition:

Aluminium oxide $(825 kg)$ , Iron $(III)$ oxide $(100 kg)$ and sand $(75 kg)$ .

What will be the percentage of Aluminium oxide in the ore, if all the Iron $(III)$ oxide is removed, leaving only the Aluminium oxide and sand?

Calculate the relative formula mass for the ionic compound hydrated Iron II sulphate, FeSO4.7H2O.

Important Questions on Reacting Masses, and Chemical Equations

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Calculate the relative formula mass for the ionic compound hydrated Iron $(II)$ sulphate, ${FeSO}_{4} . 7 H_{2} O$ .