Q.1
Which process absorbs energy?
  • Evaporation
  • Combustion
  • Neutralisation
  • Displacement
Q.2
The branch of chemistry that focuses on the study of heat released, or absorbed by chemical or physical processes is called ……………………….
  • thermochemistry
  • thermodynamics
  • thermo chemistry
  • None of these
Q.3
Heat is measured in
  • joules
  • grams
  • degrees celcius
  • mililiters
Q.4
Calorimetry Question:A piece of metal with a mass of 82.9 g is heated to 100.5°C and dropped into 71.4 g of water at 20.0°C. The final temperature of the system is 30.2°C. What is the identity of the metal?
  • Iron
  • Copper
  • Gold
  • Titanium
Q.5
H2 + Cl2 → 2 HCl +kJIs this reaction endothermic or exothermic?
  • Endothermic
  • Exothermic
Q.6
Consider the reaction: 2 H+ energy → 2H2 + O2
  • exothermic, releasing energy
  • exothemic, absorbing energy
  • endothermic, absorbing energy
  • endothermic, releasing energy
Q.7
A 16.0 g metallic sample was heated from 0°C to 35.0°C. It absorbed 248.7 J of energy. What is the identity of the metal?
  • Magnesium
  • Nickle
  • Zinc
  • Aluminium
Q.8
Calculate the amount of energy needed to convertg of ice at - 8.0 °C to steam at 150.°C.
  • 833 kJ
  • 165 kJ
  • 782 kJ
  • 251 kJ
Q.9
The thermochemical equation for precipitation of lead (II) sulphate is as follows: Pb2++SO4 −> PbSO4Pb^{2+}+SO_{^{ }}^{2-}\ \ ->\ \ PbSO_4Pb2++SO4 2−​ −> PbSO ΔH = −65.5 kJmol−1\Delta H\ =\ -65.kJmol^{-1}ΔH = −65.5 kJmol−Calculate the temperature change when 100cm3 of 0.5moldm−3100cm^of\ 0.5moldm^{-3}100cm3 of 0.5moldm−lead (II) nitrate solution is added to cm3of 0.5 moldm−cm^{3^{ }}of\ 0.moldm^{-3}cm3of 0.5 moldm−potassium sulphate solution
  • 3.9  \degree C°C
  • 4.2  \degree C°C
  • 1.9  \degree C°C
  • 2.8  $\degree C$
Q.10
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.
Q.11
How much heat is required to vaporizeg of water at 100∘C?
  • 62.7 kJ
  • 50.1 kJ
  • 150. kJ
  • 339 kJ
Q.12
What is latent heat?
  • heat that cause a temperature increase
  • heat that causes a temperature decrease
  • heat used/released in a phase change
  • large heat
Q.13
How much heat is required to melt 26.0 g of ice at 0∘C?
  • 5.88 x 104 kJ
  • 8.68 kJ
  • 109 J
  • 0 kJ
Q.14
Endothermic reactions feel
  • warm
  • cold
Q.15
Exothermic reactions feel
  • warm
  • cold
Q.16
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
Q.17
Heat flows from
  • cold to hot
  • upstream
  • freezing to boiling
  • hot to cold
Q.18
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
Q.19
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.g?
  • 1881 J
  • 250. J
  • 173 J
  • 359 J
Q.20
In an experiment,cm3 of dilute hydrochloric acid solution is mixed withcm3 sodium hydroxide solution in a polystyrene cup. The concentrations of the two solutions are the same. During the mixing, the temperature of the mixture increased by 7 0C.What is the heat released in the experiment?Given that the specific heat capacity of the solution is 4.2 J g-1 0C-1.
  • 1470 J
  • 2940 J
  • 4410 J
  • 5880 J
0 h : 0 m : 1 s