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 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 .

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 will be the total volume of gas (at rtp) from exploding 1 Kg of nitroglycerine?

Gram M r or mass of one mole of nitroglycerine is 227 g . Number of moles of nitroglycerine in 1 Kg = 1000 g 227 g ≈ 4 . 41 mol 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. Moles of gas produced in the explosion of 4 . 41 mol of nitroglycerine = 4 . 41 × 4 . 75 = 20 . 95 mol Volume of one mole of gas at rtp = 24 dm 3 Therefore, volume of 20 . 95 mole of gas at rtp = 20 . 95 mol × 24 dm 3 = 502 . 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 ) Try to explain why nitroglycerine is used as an explosive.

Since, one Kg of nitroglycerine can produce 502 . 8 dm 3 of gas. It has high nitrogen content and oxygen that can oxidise hydrogen and carbon meanwhile, nitrogen is liberated. This is a highly explosive reaction that creates high gas pressure and liberates heat which is why it is an exothermic reaction.

Nitrogen monoxide reacts with oxygen like this: 2 NO ( g ) + O 2 ( g ) → 2 NO 2 ( g ) How many moles of oxygen molecules react with 1 mol of nitrogen monoxide molecules?

Nitrogen monoxide reacts with oxygen like this: 2 NO ( g ) + O 2 ( g ) → 2 NO 2 ( g ) From the equation, it is clear that one mole of oxygen reacts with two moles of nitrogen monoxide. Therefore, half a mole of oxygen will react with one mole of nitrogen monoxide to give one mole of nitrogen dioxide.

Nitrogen monoxide reacts with oxygen like this: 2 NO ( g ) + O 2 ( g ) → 2 NO 2 ( g ) What volume of oxygen will react with 50 cm 3 of nitrogen monoxide?

Nitrogen monoxide reacts with oxygen like this: 2 NO ( g ) + O 2 ( g ) → 2 NO 2 ( g ) From the equation, it is clear that one mole of oxygen reacts with two moles of nitrogen monoxide. Therefore 25 Cm 3 of oxygen gas will react with 50 Cm 3 of nitrogen monoxide.

Nitrogen monoxide reacts with oxygen like this: 2 NO ( g ) + O 2 ( g ) → 2 NO 2 ( g ) What is the total volume of the two reactants, if nitrogen monoxide 50 cm 3 ?

Nitrogen monoxide reacts with oxygen like this: 2 NO ( g ) + O 2 ( g ) → 2 NO 2 ( g ) From the equation, it is clear that one mole of oxygen reacts with two moles of nitrogen monoxide. Therefore 25 Cm 3 of oxygen gas will react with 50 Cm 3 of nitrogen monoxide. Hence, the total volume of the reactants is 75 Cm 3 .

EASY

Upper Secondary: IGCSE

IMPORTANT

Earn 100

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?

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 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? $[A_{r} : H = 1, C = 12, N = 14, O = 16]$

HARD

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 will be the total volume of gas (at rtp) from exploding $1 Kg$ 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:

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

Try to explain why nitroglycerine is used as an explosive.

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 4

Nitrogen monoxide reacts with oxygen like this:

$2 NO (g) + O_{2} (g) \to 2 {NO}_{2} (g)$

How many moles of oxygen molecules react with $1 mol$ of nitrogen monoxide molecules?

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 4

Nitrogen monoxide reacts with oxygen like this:

$2 NO (g) + O_{2} (g) \to 2 {NO}_{2} (g)$

What volume of oxygen will react with

50 {cm}^{3}

of nitrogen monoxide?

EASY

Upper Secondary: IGCSE

IMPORTANT

Complete Chemistry for Cambridge IGCSE® Second Edition>Chapter 6 - Using Moles>Checkup on Chapter 6>Q 4

Nitrogen monoxide reacts with oxygen like this:

$2 NO (g) + O_{2} (g) \to 2 {NO}_{2} (g)$

What is the total volume of the two reactants, if nitrogen monoxide

50 {cm}^{3}

Nitroglycerine is used as an explosive. The equation for the explosion reaction is: 4C3H5(NO3)3 (l)→12CO2 (g) + 10H2O (l) + 6N2 (g) + O2 (g) How many moles does the equation show for the gas molecules produced?

Important Questions on Using Moles

Learn and Prepare for any exam you want !

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?