Quiz  /  Heat of Reaction Class 10 MCQ Questions With Answers

  • 1. 
    Neutralisation reactions

  • endothermic
  • exothermic

  • 2. 
    What is the formula for calculating heat?

  • H = mc θ\thetaθ
  • H = ΔH x n
  • H = ΔH x mass
  • products - reactants

  • 3. 
    In an experiment, 2 g of magnesium powder are added to 50 cm3 of 0.2 mol dm–3 zinc sulphate solution. The temperature of the mixture increases by 12°C. What is the heat of displacement in this experiment?[Spesific heat capacity of a solution = 4.2 Jg–1 °C–1; Relative atomic mass of Mg = 24]

  • – 50.4 kJ mol-1
  • – 100 kJ mol-1
  • – 252 kJ mol-1
  • – 340 kJ mol-1

  • 4. 
    Which of the following regarding an endothermic reaction is correct?

  • Chemical energy is transformed to heat energy
  • The temperature of the surroundings rises
  • Heat is released
  • The energy content of the product is higher than the energy content of the reactants

  • 5. 
    The ______________is required to break the bonds of the reactants.

  • Carbonic energy
  • Activation energy
  • Plutonic energy
  • Energi Gaib

  • 6. 
    What sort of reaction happens when an acid and an alkali are mixed?

  • Neutralisation
  • Combination
  • Acidifying
  • Displacement

  • 7. 
    The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?

  • Red, because the activation energy is larger
  • Blue, because the activation energy is lower
  • both reaction progress at the same rate

  • 8. 
    Compound P is dissolved in water in a test tube. It is noted that the wall of the test tube becomes cold. Which of the following is most probably compound P?

  • Sulphuric acid
  • Ammonia
  • Hydrochloride Acid
  • Ammonium chloride

  • 9. 
    At which point is the substance a solid?

  • A
  • C
  • E
  • B

  • 10. 
    What is the latent heat of fusion?

  • 4.6 kJ
  • 838.4 kJ
  • 10.15 kJ
  • 3.0 kJ

  • 11. 
    Which of the following pairs of solutions has the same heat of precipitation as the reaction between lead (II) nitrate and hydrochloric acid?

  • Barium chloride and sodium sulphate
  • Calcium chloride and sodium carbonate
  • ammonium chloride and silver nitrate
  • copper (II) chloride and lead (II) nitrate

  • 12. 
    Calculate the amount of energy needed to convert 250. g of ice at - 8.0 °C to steam at 150.°C.

  • 833 kJ
  • 165 kJ
  • 782 kJ
  • 251 kJ

  • 13. 
    A chemical reaction that absorbs heat from the surroundings is said to be __________ and has a __________ ΔH at constant pressure.

  • endothermic; positive
  • endothermic; negative
  • exothermic; negative
  • exothermic; positive

  • 14. 
    In an exothermic reaction:

  • ΔH is positive because energy is gained
  • ΔH is negative because energy is gained
  • ΔH is positive because energy is lost
  • ΔH is negative because energy is lost

  • 15. 
    Exothermic reactions feel

  • warm
  • cold

  • 16. 
    Ionic equation for precipitation of silver chloride is shown below: Ag+Ag^+Ag+ + Cl−Cl^-Cl− --> AgClWhich of the following statement is correct when defining heat of precipitation based on the chemical reaction.

  • Heat of precipitation is the heat change when 1 mol of precipitate is form from its ions.
  • Heat of precipitation is the heat change when precipitate is form from its ions.
  • Heat of precipitation is the heat change when 1 mol of silver chloride is form from silver ion and chloride ion.
  • Heat of precipitation is the heat change when silver chloride is form from silver ion and chloride ion.

  • 17. 
    Consider the reaction: 2 H2O + energy → 2H2 + O2

  • exothermic, releasing energy
  • exothemic, absorbing energy
  • endothermic, absorbing energy
  • endothermic, releasing energy

  • 18. 
    Endothermic reactions feel

  • warm
  • cold

  • 19. 
    How much heat is required to vaporize 150. g of water at 100∘C?

  • 62.7 kJ
  • 50.1 kJ
  • 150. kJ
  • 339 kJ

  • 20. 
    During a phase change, the temperature...

  • Increases
  • Decreases
  • Does nothing
  • Fluctuates

  • 21. 
    How much heat is required to raise the temperature of a sample of copper from 10.0°C to 55.0°C, if its mass is 10.00 g?

  • 1881 J
  • 250. J
  • 173 J
  • 359 J

  • 22. 
    What would be the effect on the particles if more heat is supplied to the system?

  • They would slow down
  • They would stop moving
  • They would speed up
  • There would be no effect

  • 23. 
    H2 + Cl2 → 2 HCl + 1845 kJIs this reaction endothermic or exothermic?

  • Endothermic
  • Exothermic

  • 24. 
    The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius is ________

  • Heat energy
  • Specific heat
  • convection
  • thermal energy

  • 25. 
    The following equation shows the reaction between Ag+Ag^+Ag+ and Cl−Cl^-Cl− ions. Ag+Ag^+Ag+ + Cl−Cl^-Cl− -> AgCl Δ\DeltaΔ H= -65 kJmol−1kJmol^{-1}kJmol−1 Which of the following is true about the above equation?

  • Exothermic reaction occurs
  • Heat is absorbed from the surrounding
  • The energy content of the reactants is less than the products
  • 65 kJ of heat is absorbed when 1 mole of silver chloride is formed

  • 26. 
    What is labelled "B" on the graph?

  • solids
  • liquids
  • gases
  • a phase change

  • 27. 
    Heat flows from

  • cold to hot
  • upstream
  • freezing to boiling
  • hot to cold

  • 28. 
    What letter represents a liquid being heated?

  • A
  • B
  • C
  • D

  • 29. 
    The thermochemical equation for precipitation of lead (II) sulphate is as follows: Pb2++SO4 2− −> PbSO4Pb^{2+}+SO_{4\ ^{ }}^{2-}\ \ ->\ \ PbSO_4Pb2++SO4 2−​ −> PbSO4​ ΔH = −65.5 kJmol−1\Delta H\ =\ -65.5\ kJmol^{-1}ΔH = −65.5 kJmol−1 Calculate the temperature change when 100cm3 of 0.5moldm−3100cm^3\ of\ 0.5moldm^{-3}100cm3 of 0.5moldm−3 lead (II) nitrate solution is added to 100 cm3of 0.5 moldm−3100\ cm^{3^{ }}of\ 0.5\ moldm^{-3}100 cm3of 0.5 moldm−3 potassium sulphate solution

  • 2.8  °C\degree C°C
  • 3.9  \degree C°C
  • 4.2  \degree C°C
  • 1.9  \degree C°C

  • 30. 
    Heat is measured in

  • joules
  • grams
  • degrees celcius
  • mililiters
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