Subjects

IB Chemistry HL - 2024 - Questionbank

1.3 - Reacting Masses and Volumes

Experimental, Percentage & Theoretical Yields, Limiting Reagent, Avogadro's Law, Ideal Gas Equation, Real Gases

Question Type

Paper

Paper 1
Paper 2

Difficulty

Easy
Medium
Hard

View

Question 1

no calculator

easy

What do you call the maximum amount of product that would result from the complete consumption of the limiting reagent?

  • A.\hspace{1em} Actual yield

  • B.\hspace{1em} Experimental yield

  • C.\hspace{1em} Percent yield

  • D.\hspace{1em} Theoretical yield

easy

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 2

no calculator

easy

For a fixed mass of gas at a constant temperature, what happens to the volume if the pressure of the gas is doubled?

  • A.\hspace{1em}Volume will remain the same

  • B.\hspace{1em}Volume will double

  • C.\hspace{1em}Volume will be halved

  • D.\hspace{1em}Volume will increace exponentially

easy

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 3

no calculator

easy

Which of the following conditions makes gases deviate from ideal behavior?

  • A.\hspace{1em} High pressure and high temperature

  • B.\hspace{1em} Low pressure and low temperature

  • C.\hspace{1em} High pressure and low temperature

  • D.\hspace{1em} Low pressure and high temperature

easy

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 4

no calculator

easy

Nitrogen gas reacts with hydrogen gas to produce ammonia as per the following chemical equation:

NX2(g)+3HX2(g)2NHX3(g)\ce{N2(g) + 3H2(g) -> 2NH3(g)}

If 0.86 moles\textit{moles} of NX2\ce{N2} are mixed with 0.50 moles\textit{moles} of HX2\ce{H2}, which reactant is in excess?

  • A.\hspace{1em} NX2\ce{N_{2}}

  • B.\hspace{1em} HX2\ce{H_{2}}

  • C.\hspace{1em} NHX3\ce{NH_{3}}

  • D.\hspace{1em} Both reactants are in excess

easy

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 5

no calculator

easy

What is the correct order of steps when performing titration?

  • I.\hspace{1em}Add the indicator to the flask
    II.\hspace{1em}Prepare the standard solution
    III.\hspace{1em}Swirl the flask while titrating
    IV.\hspace{1em}Fill the burette with the titrant
    V.\hspace{1em}Observe the endpoint
  • A.\hspace{1em}IV, I, III, II, V

  • B.\hspace{1em}IV, II, III, I, V

  • C.\hspace{1em}II, IV, I, III, V

  • D.\hspace{1em}II, IV, III, I, V

easy

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 6

no calculator

easy

Refer to the following chemical equation: 2NOX2(g)NX2OX4(g)\ce{2NO2 (g) -> N2O4 (g)}

At the same temperature and pressure, 25.0 cm3\textit cm^3 of nitrogen dioxide (NOX2\ce{NO2}) gas is completely converted to dinitrogen tetroxide (NX2OX4\ce{N2O4}) gas. What will be the volume of NX2OX4\ce{N2O4} produced?

  • A.\hspace{1em}10.0 cm3\textit cm^3

  • B.\hspace{1em}12.5 cm3\textit cm^3

  • C.\hspace{1em}25.0 cm3\textit cm^3

  • D.\hspace{1em}50.0 cm3\textit cm^3

easy

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 7

no calculator

easy

Based on the graph below, choose the correct statement that describes the relationship between pressure and temperature for a fixed mass and volume of a gas?

1.3-36

  • A.\hspace{1em}Pressure is inversely proportional to the absolute temperature

  • B.\hspace{1em}Pressure is directly proportional to the square of the absolute temperature

  • C.\hspace{1em}Pressure is inversely proportional to the square of the absolute temperature

  • D.\hspace{1em}Pressure is directly proportional to the absolute temperature

easy

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 8

no calculator

easy

14.01g14.01\,g of nitrogen gas (NX2\ce{N2}) is reacted with excess HX2\ce{H2}. What volume of ammonia (NHX3\ce{NH3}) gas would be produced at STP? The molar volume of a gas at STP is 22.7dm322.7 \,dm^3.

NX2(g)+3HX2(g)2NHX3(g)\ce{N2(g) + 3H2(g) -> 2NH3(g)}

  • A.\hspace{1em} 11.4dm311.4\, dm^3

  • B.\hspace{1em} 22.7dm322.7\, dm^3

  • C.\hspace{1em} 34.1dm334.1\, dm^3

  • D.\hspace{1em} 45.4dm345.4\, dm^3

easy

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 9

no calculator

easy

When a solution of lead (II) nitrate is mixed with a solution of potassium hydroxide, a precipitate containing lead (II) ions forms.

Which ions are considered to be the spectator ions?

  • A. \hspace{1em} Pb2+^{2+}, NO3_3^-

  • B. \hspace{1em} K+^+, OH^-

  • C. \hspace{1em} Pb2+^{2+}, OH^-

  • D. \hspace{1em} K+^+, NO3_3^-

easy

Formula Booklet

Mark Scheme

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Revisit

Ask Newton

Question 10

no calculator

easy

When balanced, what is the sum of the coefficients for the equation below with the lowest whole-number ratio?

BL\underline{\textrm{\htmlStyle{color: white;}{BL}}} NOX2(g)\ce{NO_2\left(g\right)} + BL\underline{\textrm{\htmlStyle{color: white;}{BL}}} HX2O(l) \ce{H2O\left(l\right)\ \rightarrow} BL\underline{\textrm{\htmlStyle{color: white;}{BL}}} HNOX3 (aq)\ce{HNO3\ \left(aq\right)} + BL\underline{\textrm{\htmlStyle{color: white;}{BL}}} NO (g)\ce{NO\ (g)}


  • A. \hspace{1em} 4

  • B. \hspace{1em} 6

  • C. \hspace{1em} 7

  • D. \hspace{1em} 5

easy

Formula Booklet

Mark Scheme

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Revisit

Ask Newton

Question 11

calculator

medium

[Maximum mark: 15]

A solution of an unknown hydrate of calcium chlorate (Ca(ClO3_3)2_2 \cdotp n H2_2O) is made by dissolving 4.164 gg in 150.0 cm3^3 of water. The resulting solution of calcium chlorate has a concentration of 0.1142 mol dm3mol \ dm^{-3}.

    1. Determine the number of moles and the mass of calcium chlorate present in the solution. [2]

    2. Determine the mass of water and then the number of moles of water that was present in the hydrate used to make the original solution. [2]

    3. Determine the value of n in the hydrate formula, Ca(ClO3_3)2_2 \cdotp n H2_2O. [1]

  1. The calcium chlorate solution made above is then mixed with 200.0 cm3cm^3 of 0.07500 mol dm30.07500 \ mol \ dm^{-3} sodium phosphate (Na3_3PO4_4 ), producing a precipitate of calcium phosphate, Ca3_3(PO4_4)2_2.

    1. Write the net ionic equation for this reaction, including state symbols. [2]

    2. Determine the limiting reactant in this reaction, showing your work. [2]

    3. If 1.535 gg of calcium phosphate is recovered, determine the percent yield in this reaction. [3]

    4. Determine the concentration of phosphate ions remaining in the solution after removing the precipitate, assuming that is the only loss of phosphate ions. [3]

medium

Formula Booklet

Mark Scheme

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Revisit

Ask Newton

Question 12

calculator

medium

[Maximum mark: 8]

The ideal gas equation is a formula that combines the relationship between pressure, volume, temperature, and the number of moles.

  1. Complete the table below by calculating the missing variables of the ideal gas equation. [4]
P\mathbf{P}V\mathbf{V}n\mathbf{n}T\mathbf{T}
(1)0.015m3\quad 0.015\, m^{3}\quad0.400mol0.400\, mol37C37 ^\circ \mathrm{C}
152,000Pa\quad 152,000\, Pa\quad(2)2.00mol2.00\, mol298.15K\quad 298.15\, K\quad
31,000Pa31,000\, Pa0.25m30.25\, m^{3}(3)271.15K271.15\, K
250kPa250\,kPa0.75dm30.75\, dm^{3}0.580mol\quad 0.580\, mol\quad(4)
  1. A 256cm3256\, cm^{3} flask contains 0.800g0.800\, g of a gaseous compound with an empirical formula of CHCl. The pressure and the temperature of the gas are respectively 105Pa10^{5}\, Pa and 373K373\, K. Determine the molecular formula of the compound. [4]

medium

Formula Booklet

Mark Scheme

Video (a)

Video (b)

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 13

calculator

medium

[Maximum mark: 4]

Liquid butanol (C4_4H9_9OH) burns or combusts in oxygen to produce CO2(g)_{2(g)} and H2_2O(g){(g)}.

  1. Write a balanced equation, including state symbols, for this reaction. [1]

  2. When 1.250 cm3cm^3 of butanol is combusted in excess oxygen, 1.921 dm3dm^3 of water vapor is collected at a pressure of 125.0 kPakPa and 150.0°\degreeC. Calculate the moles of butanol that were combusted. [2]

  3. Determine the density of liquid butanol in g cm3g \ cm^{-3}. [1]

medium

Formula Booklet

Mark Scheme

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Revisit

Ask Newton

Question 14

no calculator

medium

What is the molarity of a solution containing 7.45g7.45\, g of KCl dissolved in 250cm3250\, cm^3 solution?

  • A.\hspace{1em} 0.10moldm30.10\, mol\, dm^{-3}

  • B.\hspace{1em} 0.149moldm30.149\, mol\, dm^{-3}

  • C.\hspace{1em} 0.40moldm30.40\, mol\, dm^{-3}

  • D.\hspace{1em} 0.025moldm30.025\, mol\, dm^{-3}

medium

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 15

calculator

medium

[Maximum mark: 4]

Methanol, CHX3OH\ce{CH3OH}, is a good fuel formed by the hydrogenation of carbon monoxide according to the following chemical equation:

COX(g)+2HX2(g)CHX3OHX(l)\ce{CO_{(g)} + 2 H_{2(g)}->CH3OH_{(l)}}

  1. If 600g600\, g of CO reacts with an excess of HX2\ce{H2}, calculate the theoretical yield for methanol. [3]

  2. Determine the percentage yield if the reaction has formed 485g485\, g of CHX3OH\ce{CH3OH}. [1]

medium

Formula Booklet

Mark Scheme

Video (a)

Video (b)

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 16

no calculator

medium

Based on the table below, what is the correct calculation to determine the final volume of a fixed mass of gas:


InitialFinal
Pressure = 1.00 atm\textit atmPressure = 1.60 atm\textit atm
Temperature = 20C20^\circ\mathrm{C}Temperature = 10C10 ^\circ\mathrm{C}
Volume = 5.00 dm3\textit dm^3Volume = ?
  • A.\hspace{1em} (1.00atm)(5.00dm3)(283K)(1.60atm)(293K)\dfrac{(1.00 \textit atm)(5.00\textit dm^3)(283\textit K)}{(1.60\textit atm)(293\textit K)}

  • B.\hspace{1em} (1.00atm)(5.00dm3)(10C)(1.60atm)(20C)\dfrac{(1.00 \textit atm)(5.00\textit dm^3)(10 ^\circ\mathrm{C})}{(1.60 \textit atm)(20 ^\circ\mathrm{C})}

  • C.\hspace{1em} (1.60atm)(5.00dm3)(20C)(1.00atm)(10C)\dfrac{(1.60 \textit atm)(5.00\textit dm^3)(20 ^\circ\mathrm{C})}{(1.00 \textit atm)(10 ^\circ\mathrm{C})}

  • D.\hspace{1em} (1.60atm)(5.00dm3)(283K)(1.00atm)(293K)\dfrac{(1.60 \textit atm)(5.00\textit dm^3)(283\textit K)}{(1.00 \textit atm)(293\textit K)}

medium

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 17

calculator

medium

[Maximum mark: 3]

Automobile airbags are inflated with NX2\ce{N2}, a byproduct of sodium azide decomposition, according to the following reaction.

2NaNX3(s)2NaX(s)+3NX2(g)\ce{2 NaN_{3(s)} -> 2 Na_{(s)} + 3 N_{2(g)}}

Calculate the mass (in grams) of sodium azide needed to generate 0.07m30.07 \,m^{3} of NX2\ce{N2} at 1.01×105Pa1.01 \times 10^{5} \,Pa and 26.0°C26.0 °C.

medium

Formula Booklet

Mark Scheme

Video

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 18

no calculator

medium

The pressure of a volume V1V_1 of oxygen gas is 1.00× 105 Pa1.00 \times\ 10^5\ Pa. At constant temperature, what becomes the pressure if V1V_1 is halved?


  • A. \hspace{1em} 2.00×105 Pa2.00 \times 10^5\ Pa

  • B. \hspace{1em} 5.00×104 Pa5.00 \times 10^4\ Pa

  • C. \hspace{1em} 5.00×105 Pa5.00 \times 10^5\ Pa

  • D. \hspace{1em} 2.00×104 Pa2.00 \times 10^4\ Pa

medium

Formula Booklet

Mark Scheme

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Revisit

Ask Newton

Question 19

calculator

medium

[Maximum mark: 6]

Avogadro’s law describes the relationship between the volume of gases and the number of moles measured at the same pressure and temperature.

  1. Draw a graph that shows the variation of V\,V as n\,n changes. [1]

  2. A sample of nitrogen gas contains 1.78moles1.78\, moles and occupies a volume of 2.60dm32.60\, dm^{3} at room temperature. Determine the number of moles of the NX2\ce{N2} gas if it occupies a volume of 3.50dm33.50\, dm^{3}. [1]

  3. 15.0g15.0\, g of OX2\ce{O2} gas occupies a volume of 6.20dm36.20\, dm^{3}. Calculate the volume occupied by 30.0g30.0\, g of OX2\ce{O2} at the same temperature and pressure. [2]

  4. Calculate the volume occupied by 50.0g50.0\, g of COX2\ce{CO2} at STP. [2]

medium

Formula Booklet

Mark Scheme

Video (a)

Video (b)

Video (c)

Video (d)

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Solutions

Revisit

Ask Newton

Question 20

calculator

medium

[Maximum mark: 11]

Siderite is a mineral containing iron in the form of iron (II) carbonate, FeCO3_3.

A 15.00 gg sample of impure siderite was ground into a fine powder and dissolved in 250.0 cm3cm^3 of hot water, and then filtered to remove the insoluble components. After filtration, a 35.00 cm3cm^3 sample of the iron solution was analyzed via redox titration using a 0.120 mol dm3mol \ dm^{-3} solution of potassium dichromate. The balanced redox equation is given below:

Cr2_2O7(aq)2_{7(aq)} ^{2-} + 14 H(aq)+^+_{(aq)} + 6 Fe(aq)2+^{2+}_{(aq)} \rightarrow 2 Cr(aq)3+^{3+}_{(aq)} + 6 Fe(aq)3+^{3+}_{(aq)} + 7 H2_2O(l)_{(l)}

    1. Calculate the theoretical percent composition of iron in a sample of pure siderite or iron (II) carbonate. [1]

    2. If 18.1 cm3cm^3 of dichromate solution is used to titrate the actual iron sample to the equivalence point, calculate the number of moles of iron in the titrated sample. [2]

    3. Using your value from (ii), determine the mass of iron present in the original sample of siderite. [2]

    4. Using the experimental number of moles of FeX2+\ce{Fe^{2+}} found in (ii), calculate the experimental mass of iron carbonate (FeCO3_3) in the impure sample and then calculate the percent of impurities found in this sample. [2]

  1. Another iron-containing mineral is a hydrate of iron sulfate, Fex_x(SO4_4)y_y \cdotp nH2n H_2O, pure sample is first heated to drive off all of the water. After heating to a consistent mass, a sample with a mass of 5.250 gg is found to have 3.561 gg of anhydrous material remaining. The remaining anhydrous material was analyzed and found to have 36.76%\% iron, 21.11%\% sulfur, and 42.13%\% oxygen.

    1. Determine the empirical formula of the anhydrate. [1]

    2. If the molar mass of the hydrate is determined to be 151.92 g mol1g \ mol^{-1}, what is the actual formula of the anhydrate? [1]

    3. Use the information given in part b(i) to determine the number of moles of water present and, thus, the formula of the hydrate. [2]

medium

Formula Booklet

Mark Scheme

Revisit

Check with RV Newton

Formula Booklet

Mark Scheme

Revisit

Ask Newton

Thank you Revision Village Members

#1 IB Math Resource

Revision Village is ranked the #1 IB Math Resources by IB Students & Teachers.

34% Grade Increase

Revision Village students scored 34% greater than the IB Global Average in their exams (2021).

80% of IB Students

More and more IB students are using Revision Village to prepare for their IB Math Exams.

Frequently Asked Questions

The IB Chemistry HL Questionbank is a comprehensive set of IB Chemistry exam style questions, categorised into syllabus topic and concept, and sorted by difficulty of question. The bank of exam style questions are accompanied by high quality step-by-step markschemes and video tutorials, taught by experienced IB Chemistry teachers. The IB Chemistry HL Question bank is the perfect exam revision resource for IB students looking to practice IB Chemistry exam style questions in a particular topic or concept in their IB Chemistry Higher Level course.

The IB Chemistry HL Questionbank is designed to help IB students practice Chemistry HL exam style questions in a specific topic or concept. Therefore, a good place to start is by identifying a concept that you would like to practice and improve in and go to that area of the Chemistry HL Question bank. For example, if you want to practice Chemistry HL exam style questions covering Electron Configuration, you can go to Chemistry HL Topic 2 (Atomic Structure) and go to the Electron Configuration area of the question bank. On this page there is a carefully designed set of IB Chemistry HL exam style questions, progressing in order of difficulty from easiest to hardest. If you’re just getting started with your revision, you could start at the top of the page with the easiest questions, or if you already have some confidence, you could start at the medium difficulty questions and progress down.

The Chemistry HL Questionbank is perfect for revising a particular topic or concept, in-depth. For example, if you wanted to improve your knowledge of Electron Configuration, there are over 20 IB Chemistry HL exam style questions focused specifically on this concept. Alternatively, Revision Village also has an extensive library of Chemistry HL Practice Exams, where students can simulate the length and difficulty of an IB exam with the Mock Exam sets, as well as Chemistry HL Key Concepts, where students can learn and revise the underlying theory, if missed or misunderstood in class.

With an extensive and growing library of full length IB Chemistry HL exam style questions in the Chemistry HL Question bank, finishing all of the questions would be a fantastic effort, and you will be in a great position for your final exams. If you were able to complete all the questions in the Chemistry HL Question bank, then a popular option would be to go to the Chemistry HL Practice Exams section on Revision Village and test yourself with the Mock Exam Papers, to simulate the length and difficulty of an actual IB Chemistry HL exam.