Give all answers to 3 significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows: NH 4 NO 3 s → N 2 O g + 2 H 2 O l ( A r values: N = 14 . 0 , H = 1 . 0 , O = 16 . 0 ). How many moles of ammonium nitrate are present in 0 . 800 g of the solid?

1 mole is number which is equal to 6 . 022 × 10 23 particles, also known as the Avogadro's constant. These particles can be any type of species, e.g atoms, molecules, electrons, protons, neutron NH 4 NO 3 s → N 2 O g + 2 H 2 O l Molar mass of ammonium nitrate, from given A r values = 2 × 14 + 1 × 4 + 3 × 16 = 80 g / mol Mass of ammonium nitrate = 0 . 800 g Moles of ammonium nitrate = Mass Molar mass = 0 . 800 80 . 0 = 0 . 01 mol

Give all answers to 3 significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows: NH 4 NO 3 s → N 2 O g + 2 H 2 O l ( A r values: N = 14 . 0 , H = 1 . 0 , O = 16 . 0 ). Calculate the volume of N 2 O gas that would be produced from 0 . 800 g mass of ammonium nitrate?

1 mole is number which is equal to 6 . 022 × 10 23 particles, also known as the Avogadro's constant. These particles can be any type of species, e.g atoms, molecules, electrons, protons, neutron NH 4 NO 3 s → N 2 O g + 2 H 2 O l From the above balanced equation, 1 mole of ammonium nitrate undergone to give 1 mole of N 2 O . We have asked to calculate how much of N 2 O gas released = ? Molar mass of ammonium nitrate, from given A r values = 2 × 14 + 1 × 4 + 3 × 16 = 80 g / mol Mass of ammonium nitrate = 0 . 800 g Moles of ammonium nitrate = Mass Molar mass = 0 . 800 80 . 0 = 0 . 01 mol So 0 . 01 mole of ammonium nitrate gives 0 . 01 mole of N 2 O gas. Volume of N 2 O gas dm 3 = Number of moles × 24 . 0 = 0 . 01 × 24 . 0 = 0 . 24 dm 3

Give the answer to 3 significant figures. 4 . 80 dm 3 of chlorine gas was reacted with sodium hydroxide solution. The reaction taking place was as follows: Cl 2 g + 2 NaOH aq → NaCl aq + NaOCl aq + H 2 O l . ( A r values: Na = 23 . 0 ; Cl = 35 . 5 ; O = 16 . 0 ) The concentration of the NaOH was 2 . 00 mol dm - 3 . Calculate the volume of sodium hydroxide solution required.

1 mole is number which is equal to 6 . 022 × 10 23 particles, also known as the Avogadro's constant. These particles can be any type of species, e.g atoms, molecules, electrons, protons, neutrons. Cl 2 g + 2 NaOH aq → NaCl aq + NaOCl aq + H 2 O l Volume of chlorine gas = 4 . 80 dm 3 Then, number of moles of chlorine gas = voleme ( dm 3 ) 24 . 0 = 4 . 80 24 . 0 = 0 . 2 mol From the balanced equation 1 mole of chlorine gas react with 2 moles of NaOH (sodium hydroxide) solution. Hence, moles number of NaOH is 0 . 2 mol We have given, Concentration(molarity) of NaOH = 2 . 00 mol dm - 3 Then, the volume of NaOH = Moles number Molarity = 0 . 2 2 . 00 = 0 . 1 dm 3

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Give all answers to $3$ significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows:

${NH}_{4} {NO}_{3} (s) \to N_{2} O (g) + 2 H_{2} O (l)$

( $A_{r}$ values: $N = 14.0, H = 1.0, O = 16.0$ ).

Deduce the formula mass of ammonium nitrate.

Important Questions on Atoms, Molecules and Stoichiometry

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AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 3 - Atoms, Molecules and Stoichiometry>EXAM-STYLE QUESTIONS>Q 7

Give all answers to $3$ significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows:

${NH}_{4} {NO}_{3} (s) \to N_{2} O (g) + 2 H_{2} O (l)$

( $A_{r}$ values: $N = 14.0, H = 1.0, O = 16.0$ ).

How many moles of ammonium nitrate are present in $0.800 g$ of the solid?

MEDIUM

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 3 - Atoms, Molecules and Stoichiometry>EXAM-STYLE QUESTIONS>Q 7

Give all answers to $3$ significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows:

${NH}_{4} {NO}_{3} (s) \to N_{2} O (g) + 2 H_{2} O (l)$

( $A_{r}$ values: $N = 14.0, H = 1.0, O = 16.0$ ).

Calculate the volume of $N_{2} O$ gas that would be produced from $0.800 g$ mass of ammonium nitrate?

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 3 - Atoms, Molecules and Stoichiometry>EXAM-STYLE QUESTIONS>Q 8

Give all answers to $3$ significant figures. $1.20 {dm}^{3}$ of hydrogen chloride gas was dissolved in $100 {cm}^{3}$ of water.

i. Calculate the number of moles of hydrogen chloride gas present.

ii. Calculate the concentration of the hydrochloric acid formed.

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AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 3 - Atoms, Molecules and Stoichiometry>EXAM-STYLE QUESTIONS>Q 8

Give all answers to $3$ significant figures. $25.0 {cm}^{3}$ of the acid was then titrated against sodium hydroxide of concentration $0.200 mol {dm}^{- 3}$ to form $NaCl$ and water: $NaOH + HCl \to H_{2} O + NaCl$ .

i. Calculate the number of moles of acid used.

ii. Calculate the volume of sodium hydroxide used.

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 3 - Atoms, Molecules and Stoichiometry>EXAM-STYLE QUESTIONS>Q 9

Give the answer to $3$ significant figures. $4.80 {dm}^{3}$ of chlorine gas was reacted with sodium hydroxide solution. The reaction taking place was as follows:

${Cl}_{2} (g) + 2 NaOH (aq) \to NaCl (aq) + NaOCl (aq) + H_{2} O (l)$ .

( $A_{r}$ values: $Na = 23.0; Cl = 35.5; O = 16.0$ )

Calculate the number of moles of ${Cl}_{2}$ reacted.

MEDIUM

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 3 - Atoms, Molecules and Stoichiometry>EXAM-STYLE QUESTIONS>Q 9

Give the answer to $3$ significant figures. $4.80 {dm}^{3}$ of chlorine gas was reacted with sodium hydroxide solution. The reaction taking place was as follows:

${Cl}_{2} (g) + 2 NaOH (aq) \to NaCl (aq) + NaOCl (aq) + H_{2} O (l)$ .

( $A_{r}$ values: $Na = 23.0; Cl = 35.5; O = 16.0$ )

Calculate the mass of $NaOCl$ formed.

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 3 - Atoms, Molecules and Stoichiometry>EXAM-STYLE QUESTIONS>Q 9

Give the answer to $3$ significant figures. $4.80 {dm}^{3}$ of chlorine gas was reacted with sodium hydroxide solution. The reaction taking place was as follows:

${Cl}_{2} (g) + 2 NaOH (aq) \to NaCl (aq) + NaOCl (aq) + H_{2} O (l)$ .

( $A_{r}$ values: $Na = 23.0; Cl = 35.5; O = 16.0$ )

The concentration of the $NaOH$ was $2.00 mol {dm}^{- 3}$ . Calculate the volume of sodium hydroxide solution required.

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 3 - Atoms, Molecules and Stoichiometry>EXAM-STYLE QUESTIONS>Q 9

Give the answer to $3$ significant figures. $4.80 {dm}^{3}$ of chlorine gas was reacted with sodium hydroxide solution. The reaction taking place was as follows:

${Cl}_{2} (g) + 2 NaOH (aq) \to NaCl (aq) + NaOCl (aq) + H_{2} O (l)$ .

( $A_{r}$ values: $Na = 23.0; Cl = 35.5; O = 16.0$ )

Write an ionic equation for this reaction.

Give all answers to 3 significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows: NH4NO3s→N2Og+2H2Ol (Ar values: N=14.0, H=1.0, O=16.0). Deduce the formula mass of ammonium nitrate.

Important Questions on Atoms, Molecules and Stoichiometry

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Give all answers to $3$ significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows:

${NH}_{4} {NO}_{3} (s) \to N_{2} O (g) + 2 H_{2} O (l)$

( $A_{r}$ values: $N = 14.0, H = 1.0, O = 16.0$ ).

Deduce the formula mass of ammonium nitrate.