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WorksheetsQUIZIZZ100: Thermochemistry #2
Total questions: 19
Worksheet time: 5hrs 45mins
In an exothermic reaction...
Heat is released, potential energy of reactants increases
Heat is released, potential energy of reactants decreases
Heat is absorbed, potential energy of reactants increases
Heat is absorbed, potential energy of reactants decreases
A calorimeter contains 400 ml of water at 25 oC. If 600 ml of water at 60.0 oC is added to it, determine its final temperature. Assume that the heat absorbed by the calorimeter is negligible (Density of water = 1.00 g/ml).
39.0 oC
42.5 oC
46.0 oC
52.5 oC
Based on the diagram, choose the correct statement.
The reaction shown is exothermic
The reaction shown is endothermic
The reactant loses heat to the product
The reaction is reversible
What would the final temperature of 250 ml of water at 29.0 oC if it absorbed 10.0 kJ of heat? (Density of water = 1.00 g/ml; Specific heat capacity of water = 4.18 J g-1 oC-1).
19.4 oC
29.1 oC
38.6 oC
9.6 oC
Calculate the amount of energy used to raise the temperature of 50 g of water from 28.0 oC to 50.0 oC.
4.60 kJ
5.85 kJ
10.5 kJ
62.9 kJ
Which of the following is endothermic?
I2 (l) --> I2 (s)
I2 (g) --> 2I (s)
I (g) + e --> I- (g)
I- (g) --> I- (aq)
Calculate the species heat of substance X if it takes 7.21 kJ of heat to raise 80.0 g of X by 100 oC.
9.01 x 10-4 J g-1 oC-1
0.901 J g-1 oC-1
0.20 J g-1 oC-1
5.77 J g-1 oC-1
Which equation represents the enthalpy change of atomisation of bromine?
Br2 (aq) --> 2Br (g)
1/2Br2 (g) --> Br (g)
1/2Br2 (l) --> Br (g)
Br2 (l) --> 2Br (g)
The value of ΔH° for the reaction below is -3,351 kJ.
2Al (s) + 3O2 (g) → 2Al2O3 (s)
Calculate the ΔH° for the formation of 20.0 g of aluminium oxide.
-167.6 kJ
-328.0 kJ
+246.0 kJ
-1676 kJ
If 2H2 (g) + O2 (g) --> 2H2O (g) has ΔH = −241.8 kJ. What would be the ΔH of the following?
H2O (g) --> H2 (g) + 1/2O2 (g)
-120.9 kJ
-241.8 kJ
+120.9 kJ
+241.8 kJ
If the heat capacity of lead is 0.13 J/g K. Calculate the amount energy required to raise the temperature of 10 g lead from 28 oC to 50 oC?
29 J
36 J
65 J
59 J
100 ml of an unknown liquid with a temperature of 30 oC is mixed with 80 ml of the same liquid at 50 oC. Determine the final temperature of the mixture if the density of the liquid is 0.90 g/ml. Assume that no heat is lost to the surroundings.
35.5 oC
38.9 oC
40.0 oC
80.0 oC
A piece of metal weighing 350 g is heated from 25 oC to 117 oC. Determine its specific heat if it is found to have absorbed 12.5 kJ of heat.
0.128 J g-1 oC-1
0.305 J g-1 oC-1
0.388 J g-1 oC-1
4.18 J g-1 oC-1
Calculate the quantity of water that can be heated from 25.0 oC to 40.0 oC by the addition of 1000 J of energy.
15.9 g
62.7 g
102 g
239 g
Which of the following elements standard enthalpy of atomisation would have the same value as its enthalpy of vapourisation?
Na
Hg
Cl
C
All the following would be expected to have enthalpy of formation values of zero EXCEPT.
Cl2 (g)
Mg (s)
Hg (l)
C (diamond)
3.2 g of methane is burned in excess oxygen in a bomb calorimeter. The heat liberated by the combustion caused the temperature of the calorimeter to elevate by 20.9 oC. If the heat capacity of the calorimeter is 8.50 kJ oC-1, what is enthalpy of combustion of methane?
-35.6 kJ mol-1
-178 kJ mol-1
-568 kJ mol-1
-888 kJ mol-1
When 25.0 ml of 1.0 M HCl is mixed with 25.0 ml of 1.0 ml NaOH in a coffee cup calorimeter, the temperature of the solution increased by 6.8 oC. Assuming the heat loss to the calorimeter is negligible, which of the following statement is UNTRUE? (Density of water = 1.00 g/ml; Specific heat capacity of water = 4.18 J g-1 oC-1)
1.42 kJ heat were transferred during the process
For the reaction, q = +1.42 kJ
The enthalpy of neutralisation for this reaction is -56.85 kJ/mol
The reaction was exothermic
Select the statement that most accurately describes Hess's Law.
The enthalpy of a reaction depends on the physical states of both reactants and products.
When an equation is reversed, the value of enthalpy difference must also be reversed.
The value of enthalpy difference of a reaction that can be written in steps is the sum of the values of enthalpy differences for the individual steps.
Enthalpy changes occur only after the reaction achieves dynamic equilibrium.
