With strong heating, calcium carbonate undergoes thermal decomposition: CaCO 3 ( s ) → CaO ( s ) + CO 2 ( g ) Write a Word equation for the change.

With strong heating, calcium carbonate undergoes thermal decomposition: CaCO 3 ( s ) → CaO ( s ) + CO 2 ( g ) The word equation is as follows: Calcium carbonate → thermal decomposition Calcium oxide + Carbon dioxide Calcium carbonate is a reactant and the products are calcium oxide and carbon dioxide.

With strong heating, calcium carbonate undergoes thermal decomposition: CaCO 3 ( s ) → CaO ( s ) + CO 2 ( g ) Write a Word equation for the change.

With strong heating, calcium carbonate undergoes thermal decomposition: CaCO 3 ( s ) → CaO ( s ) + CO 2 ( g ) The word equation is as follows: Calcium carbonate → thermal decomposition Calcium oxide + Carbon dioxide Calcium carbonate is a reactant and the products are calcium oxide and carbon dioxide.

With strong heating, calcium carbonate undergoes thermal decomposition: CaCO 3 ( s ) → CaO ( s ) + CO 2 ( g ) How many moles of CaCO 3 are in 50 g of calcium carbonate? A r : Ca = 40 , C = 12 , O = 16

Gram molecular mass of CaCO 3 = 40 g + 12 g + 3 × 16 g = 100 g Number of moles in its 50 g = 50 g 100 g = 0 . 5 mol

With strong heating, calcium carbonate undergoes thermal decomposition: CaCO 3 ( s ) → CaO ( s ) + CO 2 ( g ) What mass of calcium oxide is obtained from the thermal decomposition of 50 g of calcium carbonate, assuming a 40 % yield?

CaCO 3 ( s ) → CaO ( s ) + CO 2 ( g ) Gram molecular mass of CaCO 3 = 100 g and that of CaO = 56 g . From the reaction it is clear that one mol of calcium carbonate produces one mol of calcium oxide. Since, 100 g of calcium carbonate will produce 56 g of calcium oxide. Therefore 50 g of calcium carbonate will produce 28 g of calcium oxide. Since % yield is 40 % , therefore mass of calcium oxide obtained = 40 % × 28 g 100 = 11 . 2 g

With strong heating, calcium carbonate undergoes thermal decomposition: CaCO 3 ( s ) → CaO ( s ) + CO 2 ( g ) What mass of carbon dioxide will be given off from 50 g of calcium carbonate, assuming a 40 % yield? What volume will this gas occupy at rtp?

CaCO 3 ( s ) → CaO ( s ) + CO 2 ( g ) Gram molecular mass of CaCO 3 = 100 g and that of CO 2 = 44 g . From the reaction it is clear that one mol of calcium carbonate produces one mol of carbon dioxide. Since, 100 g of calcium carbonate will produce 44 g of carbon dioxide. Therefore 50 g of calcium carbonate will produce 22 g of carbon dioxide. Since % yield is 40 % , therefore mass of calcium oxide obtained = 40 % × 22 g 100 = 8 . 8 g Gram M r of CO 2 = 44 g 44 g = 1 mol Number of moles of carbon dioxide in its 8 . 8 g = 8 . 8 g 44 g = 0 . 2 mol So the volume occupied by the gas at rtp= 0 . 2 mol × 24 dm 3 = 4 . 8 dm 3

Nitroglycerine is used as an explosive. The equation for the explosion reaction is: 4 C 3 H 5 ( NO 3 ) 3 ( l ) → 12 CO 2 ( g ) + 10 H 2 O ( l ) + 6 N 2 ( g ) + O 2 ( g ) How many moles does the equation show for nitroglycerine?

4 C 3 H 5 ( NO 3 ) 3 ( l ) → 12 CO 2 ( g ) + 10 H 2 O ( l ) + 6 N 2 ( g ) + O 2 ( g ) In the above reaction, the reactant is nitroglycerine and after the explosion, the products are carbon dioxide gas, nitrogen gas, oxygen gas and water molecules. The equation shows 4 moles of nitroglycerine.

Nitroglycerine is used as an explosive. The equation for the explosion reaction is: 4 C 3 H 5 ( NO 3 ) 3 ( l ) → 12 CO 2 ( g ) + 10 H 2 O ( l ) + 6 N 2 ( g ) + O 2 ( g ) How many moles does the equation show for the gas molecules produced?

4 C 3 H 5 ( NO 3 ) 3 ( l ) → 12 CO 2 ( g ) + 10 H 2 O ( l ) + 6 N 2 ( g ) + O 2 ( g ) In the above reaction, the reactant is nitroglycerine and after the explosion, the products are carbon dioxide gas, nitrogen gas, oxygen gas and water molecules. The equation shows that 4 moles of nitroglycerine on explosion produces 12 moles of carbon dioxide gas, 6 moles of nitrogen gas and 1 mole of oxygen gas. Hence, total 19 moles of gas is formed.

Nitroglycerine is used as an explosive. The equation for the explosion reaction is: 4 C 3 H 5 ( NO 3 ) 3 ( l ) → 12 CO 2 ( g ) + 10 H 2 O ( l ) + 6 N 2 ( g ) + O 2 ( g ) How many moles of gas molecules are obtained from 1 mole of nitroglycerine?

4 C 3 H 5 ( NO 3 ) 3 ( l ) → 12 CO 2 ( g ) + 10 H 2 O ( l ) + 6 N 2 ( g ) + O 2 ( g ) Since, the equation shows that 4 moles of nitroglycerine on explosion produces 12 moles of carbon dioxide gas, 6 moles of nitrogen gas and 1 mole of oxygen gas. Therefore, one mole of nitroglycerine will produce 3 mol CO 2 , 1 . 5 mol N 2 and 0 . 25 mol O 2 . So, in total 4 . 75 mol of gas molecules are produced in the explosion.

Nitroglycerine is used as an explosive. The equation for the explosion reaction is: 4 C 3 H 5 ( NO 3 ) 3 ( l ) → 12 CO 2 ( g ) + 10 H 2 O ( l ) + 6 N 2 ( g ) + O 2 ( g ) What is the total volume of gas (at rtp) obtained from 1 mole of nitroglycerine?

4 C 3 H 5 ( NO 3 ) 3 ( l ) → 12 CO 2 ( g ) + 10 H 2 O ( l ) + 6 N 2 ( g ) + O 2 ( g ) Since, one mole of nitroglycerine will produce 3 mol CO 2 , 1 . 5 mol N 2 and 0 . 25 mol O 2 . So, in total 4 . 75 mol of gas molecules are produced in the explosion. Volume of one mole of gas at rtp = 24 dm 3 Therefore, volume of 4 . 75 mole of gas at rtp = 4 . 75 mol × 24 dm 3 = 114 dm 3

Nitroglycerine is used as an explosive. The equation for the explosion reaction is: 4 C 3 H 5 ( NO 3 ) 3 ( l ) → 12 CO 2 ( g ) + 10 H 2 O ( l ) + 6 N 2 ( g ) + O 2 ( g ) What is the mass of 1 mole of nitroglycerine? A r : H = 1 , C = 12 , N = 14 , O = 16

Since, M r of nitroglycerine = 3 × 12 u + 5 × 1 u + 3 × 14 u + 3 × 16 u = 227 u Therefore gram M r or mass of one mole of nitroglycerine is 227 g .

EASY

Upper Secondary: IGCSE

IMPORTANT

Earn 100

With strong heating, calcium carbonate undergoes thermal decomposition:

${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$

Write a Word equation for the change.

Important Questions on Using Moles

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 2

With strong heating, calcium carbonate undergoes thermal decomposition:

${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$

How many moles of ${CaCO}_{3}$ are in $50 g$ of calcium carbonate? $(A_{r} : Ca = 40, C = 12, O = 16)$

HARD

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 2

With strong heating, calcium carbonate undergoes thermal decomposition:

${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$

What mass of calcium oxide is obtained from the thermal decomposition of $50 g$ of calcium carbonate, assuming a $40 %$ yield?

MEDIUM

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 2

With strong heating, calcium carbonate undergoes thermal decomposition:

${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$

What mass of carbon dioxide will be given off from $50 g$ of calcium carbonate, assuming a $40 %$ yield?
What volume will this gas occupy at rtp?

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 3

Nitroglycerine is used as an explosive. The equation for the explosion reaction is:

$4 C_{3} H_{5} {({NO}_{3})}_{3} (l) \to 12 {CO}_{2} (g) + 10 H_{2} O (l) + 6 N_{2} (g) + O_{2} (g)$

How many moles does the equation show for nitroglycerine?

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 3

Nitroglycerine is used as an explosive. The equation for the explosion reaction is:

$4 C_{3} H_{5} {({NO}_{3})}_{3} (l) \to 12 {CO}_{2} (g) + 10 H_{2} O (l) + 6 N_{2} (g) + O_{2} (g)$

How many moles does the equation show for the gas molecules produced?

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 3

Nitroglycerine is used as an explosive. The equation for the explosion reaction is:

$4 C_{3} H_{5} {({NO}_{3})}_{3} (l) \to 12 {CO}_{2} (g) + 10 H_{2} O (l) + 6 N_{2} (g) + O_{2} (g)$

How many moles of gas molecules are obtained from $1$ mole of nitroglycerine?

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 3

Nitroglycerine is used as an explosive. The equation for the explosion reaction is:

$4 C_{3} H_{5} {({NO}_{3})}_{3} (l) \to 12 {CO}_{2} (g) + 10 H_{2} O (l) + 6 N_{2} (g) + O_{2} (g)$

What is the total volume of gas (at rtp) obtained from $1$ mole of nitroglycerine?

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 3

Nitroglycerine is used as an explosive. The equation for the explosion reaction is:

$4 C_{3} H_{5} {({NO}_{3})}_{3} (l) \to 12 {CO}_{2} (g) + 10 H_{2} O (l) + 6 N_{2} (g) + O_{2} (g)$

What is the mass of $1$ mole of nitroglycerine? $[A_{r} : H = 1, C = 12, N = 14, O = 16]$

With strong heating, calcium carbonate undergoes thermal decomposition: CaCO3(s)→CaO(s) + CO2(g) Write a Word equation for the change.

Important Questions on Using Moles

Learn and Prepare for any exam you want !

With strong heating, calcium carbonate undergoes thermal decomposition:

${CaCO}_{3} (s) \to CaO (s) + {CO}_{2} (g)$

Write a Word equation for the change.