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WorksheetsThermochemistry
Total questions: 16
Worksheet time: 14mins
During an exothermic reaction, heat content in the surroundings increases because
heat energy is destroyed during reactions
the reaction absorbs heat energy
the energy contained in the reactants is lower then the products
the energy contained in the products is lower than the reactants
Releasing heat into the surroundings occurs during an ___________________ reaction.
Exothermic
Endothermic
Kinetic Energy
Thermal Energy
Match the definition below to the correct term.
The enthalpy change that takes place when one mole of a compound is formed from its elements in their standard states under standard conditions.
The enthalpy of neutralisation
The enthalpy of combustion
The enthalpy of formation
The enthalpy of reaction
What does the circle mean in ΔH°?
Standard Conditions (T=298.15 K P=1 atm)
Standard Temperature and Pressure (T=273.15 K P=1 atm)
Degree K
Degree C
How do you calculate Enthalpy of a reaction?
ΔH = ΔHproducts - ΔHreactants
ΔT = q / mC
ΔG = ΔH -TΔS
E = mc2
"Heat change when 1 mole of gaseous atom is formed from its element at standard states" is the definition for _______.
standard enthalpy of formation
standard enthalpy ofhydration
electron affinity
standard enthalpy of atomisation
Name the type of enthalpy for the following reaction:
Na+ (g) --> Na+ (aq) ΔH = -364 kJmol-1
Standard enthalpy of neutralisation, ΔHneuto
Standard enthalpy of solution, ΔHsolno
Standard enthalpy of hydration, ΔHhydo
lattice energy, ΔHlatticeo
Define standard enthalpy of combustion.
Heat released when one mole of substance is burnt completely in excess oxygen.
Heat absorbed when one mole of substance is burnt completely in excess oxygen under standard state.
Heat released when one mole of substance is burnt completely in excess oxygen under standard state.
Heat change when one mole of substance is burnt partially in excess oxygen under standard state.
Which of the equation below refers to the standard enthalpy of formation, ΔHfo?
Na(g) ---> Na+(g) + e- ΔH = -364 kJmol-1
C2H5OH(l) + 3O2(g) ---> 2CO2(g) + 3H2O (l) ΔH = - 1286 kJmol-1
2C(s) + 2H2(g) ---> C2H4 (g) ΔH = - 52.3 kJmol-1
Na+(g) ---> Na+(aq) ΔH = - 364 kJmol-1
providing alternative pathway with lower activation energy
lowering the activation energy
A reaction that gives out energy to the surroundings causes the surroundings ....
temperature to drop
temperature to rise
temperature to remain constant
temperature to vary
Which of the following represents an exothermic reaction?
The quantity of heat needed to raise the temperature of a sample of a substance by one degree Celsius is the sample’s
Calorimeter
Specific heat capacity
Enthalpy
Heat capacity
Hess’s law states that when the reactants are converted to products, the enthalpy change of a reaction is ____ whether the reaction takes place in one step or a series of step
different
same
lower
greater
