Butane lighters work by the release and combustion of pressurised butane: 2 C 4 H 10 g + 13 O 2 g → 8 CO 2 g + 10 H 2 O l Determine the limiting reagent in the reaction, 20 molecules of C 4 H 10 and 100 molecules of O 2 .

Consider the given reaction, 2 C 4 H 10 g + 13 O 2 g → 8 CO 2 g + 10 H 2 O l . We know that, one mole of C 4 H 10 contains 6 . 02 × 10 23 molecules. Therefore, the number of moles of butane in 20 molecules = 20 6 . 02 × 10 23 = 3 . 32 × 10 - 23 mol , and The number of moles of oxygen in 100 molecules = 100 6 . 02 × 10 23 = 16 . 61 × 10 - 23 mol According to the balanced equation, 2 mol of butane requires 13 mol of oxygen. Therefore, the number of moles of oxygen required to react with 3 . 32 × 10 - 23 mol = 3 . 32 × 10 - 23 × 13 2 = 21 . 58 × 10 - 23 mol . But, only 16 . 61 × 10 - 23 mol of oxygen is available in the reaction, hence, oxygen is the limiting reagent in the reaction.

Butane lighters work by the release and combustion of pressurised butane: 2 C 4 H 10 g + 13 O 2 g → 8 CO 2 g + 10 H 2 O l Determine the limiting reagent in the reaction, 10 molecules of C 4 H 10 and 91 molecules of O 2 .

Consider the given reaction, 2 C 4 H 10 g + 13 O 2 g → 8 CO 2 g + 10 H 2 O l . We know that, one mole of C 4 H 10 contains 6 . 02 × 10 23 molecules. Therefore, the number of moles of butane in 10 molecules = 10 6 . 02 × 10 23 = 1 . 66 × 10 - 23 mol , and The number of moles of oxygen in 91 molecules = 91 6 . 02 × 10 23 = 15 . 11 × 10 - 23 mol According to the balanced equation, 2 mol of butane requires 13 mol of oxygen. Therefore, the number of moles of oxygen required to react with 1 . 66 × 10 - 23 mol = 1 . 66 × 10 - 23 × 13 2 = 10 . 79 × 10 - 23 mol . But, 15 . 11 × 10 - 23 mol of oxygen is available in the reaction, hence, butane is the limiting reagent in the reaction.

Butane lighters work by the release and combustion of pressurised butane: 2 C 4 H 10 g + 13 O 2 g → 8 CO 2 g + 10 H 2 O l Determine the limiting reagent in the reaction, 0 . 20 mol of C 4 H 10 and 2 . 6 mol of O 2 .

Consider the given reaction, 2 C 4 H 10 g + 13 O 2 g → 8 CO 2 g + 10 H 2 O l . According to the balanced equation, 2 mol of butane requires 13 mol of oxygen. Therefore, the number of moles of oxygen required to react with 0 . 20 mol of butane = 0 . 20 × 13 2 = 1 . 3 mol . But, 2 . 6 mol of oxygen is available in the reaction, hence, butane is the limiting reagent in the reaction.

Butane lighters work by the release and combustion of pressurised butane: 2 C 4 H 10 g + 13 O 2 g → 8 CO 2 g + 10 H 2 O l Determine the limiting reagent in the reaction, 8 . 72 g of C 4 H 10 and 28 . 8 g of O 2 .

Consider the given reaction, 2 C 4 H 10 g + 13 O 2 g → 8 CO 2 g + 10 H 2 O l . The amount of butane (in mol ) = 8 . 72 58 = 0 . 15 mol The amount of oxygen (in mol ) = 28 . 8 32 = 0 . 9 mol According to the balanced equation, 2 mol of butane requires 13 mol of oxygen. Therefore, the number of moles of oxygen required to react with 0 . 15 mol of butane = 0 . 15 × 13 2 = 0 . 975 mol . But, only 0 . 9 mol of oxygen is available in the reaction, hence, oxygen is the limiting reagent in the reaction.

EASY

Diploma

IMPORTANT

Earn 100

Calculate the number of particles present in $0.200 mol$ of sodium chlorate( $VII$ ), ${NaClO}_{4}$ .

Important Questions on Stoichiometric Relationships

EASY

Diploma

IMPORTANT

Oxford IB Diploma Programme Chemistry Course Companion>Chapter 1 - Stoichiometric Relationships>Quick questions>Q 3

Calculate the number of particles present in

72.99 g

of iron(

III

) chloride,

{FeCl}_{3}

EASY

Diploma

IMPORTANT

Oxford IB Diploma Programme Chemistry Course Companion>Chapter 1 - Stoichiometric Relationships>Quick questions>Q 3

Calculate the number of particles present in

4.60 g

of nitrogen(

IV

) oxide.

EASY

Diploma

IMPORTANT

Oxford IB Diploma Programme Chemistry Course Companion>Chapter 1 - Stoichiometric Relationships>TOK

Mathematics is an integral part of scientific endeavours.The use of numbers and an understanding of the mole concept have helped develop Chemistry into a physical science. Why is mathematics so effective in describing the natural world?

EASY

Diploma

IMPORTANT

Oxford IB Diploma Programme Chemistry Course Companion>Chapter 1 - Stoichiometric Relationships>Quick questions>Q 1

Butane lighters work by the release and combustion of pressurised butane:

$2 C_{4} H_{10} (g) + 13 O_{2} (g) \overset{}{\to} 8 {CO}_{2} (g) + 10 H_{2} O (l)$

Determine the limiting reagent in the reaction, $20$ molecules of $C_{4} H_{10}$ and $100$ molecules of $O_{2}$ .

EASY

Diploma

IMPORTANT

Oxford IB Diploma Programme Chemistry Course Companion>Chapter 1 - Stoichiometric Relationships>Quick questions>Q 1

Butane lighters work by the release and combustion of pressurised butane:

$2 C_{4} H_{10} (g) + 13 O_{2} (g) \overset{}{\to} 8 {CO}_{2} (g) + 10 H_{2} O (l)$

Determine the limiting reagent in the reaction, $10$ molecules of $C_{4} H_{10}$ and $91$ molecules of $O_{2}$ .

EASY

Diploma

IMPORTANT

Oxford IB Diploma Programme Chemistry Course Companion>Chapter 1 - Stoichiometric Relationships>Quick questions>Q 1

Butane lighters work by the release and combustion of pressurised butane:

$2 C_{4} H_{10} (g) + 13 O_{2} (g) \overset{}{\to} 8 {CO}_{2} (g) + 10 H_{2} O (l)$

Determine the limiting reagent in the reaction, $0.20 mol$ of $C_{4} H_{10}$ and $2.6 mol$ of $O_{2}$ .

EASY

Diploma

IMPORTANT

Oxford IB Diploma Programme Chemistry Course Companion>Chapter 1 - Stoichiometric Relationships>Quick questions>Q 1

Butane lighters work by the release and combustion of pressurised butane:

$2 C_{4} H_{10} (g) + 13 O_{2} (g) \overset{}{\to} 8 {CO}_{2} (g) + 10 H_{2} O (l)$

Determine the limiting reagent in the reaction, $8.72 g$ of $C_{4} H_{10}$ and $28.8 g$ of $O_{2}$ .

EASY

Diploma

IMPORTANT

Oxford IB Diploma Programme Chemistry Course Companion>Chapter 1 - Stoichiometric Relationships>Quick questions>Q 2

Two aqueous solutions, one containing $5.3 g$ of sodium carbonate and the other $7.0 g$ of calcium chloride, are mixed together. A precipitation reaction occurs:

${Na}_{2} {CO}_{3} (aq) + {CaCl}_{2} (aq) \overset{}{\to} {CaCO}_{3} (s) + 2 NaCl (aq)$

Determine the limiting reagent and the mass, in $g$ , of precipitate formed.

Calculate the number of particles present in 0.200 mol of sodium chlorate(VII),NaClO4.

Important Questions on Stoichiometric Relationships

Learn and Prepare for any exam you want !

Calculate the number of particles present in $0.200 mol$ of sodium chlorate( $VII$ ), ${NaClO}_{4}$ .