Thermochemistry Exam Review 2g, 6a, 6b
Quiz by Darrien James
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- Q1If a 50 g piece of an unknown metal is heated from 25 °C to 100 °C and absorbs 800 J of heat, what is the specific heat of aluminum?4.68 J/g °C1200 J/g °C0.480 J/g °C0.213 J/g °C30s
- Q2What does 'q' represent in the q=mcΔT formula?ForceMassHeat energyVelocity30s
- Q3What does 'c' represent in the q=mcΔT formula?Coefficient of frictionSpeed of lightConcentrationSpecific heat30s
- Q4
Open the image below and respond to the question:
+73 kJ
-73 kJ
-53 kJ
+53 kJ
30s - Q5
Open the image below and answer the question:
-168 kJ
-8kJ
+168 kJ
+8 kJ
30s - Q6
Examine the table:
A 5g ring of each metal was heated with 100J of energy, which of the four metal rings will have the greatest temperature change?
The titanium ring, because it has the highest specific heat, therefore it requires the least energy to increase the temperature of the ring by 1°C.
The tin ring, because it has the lowest specific heat, therefore it requires the least energy to increase the temperature of the ring by 1°C.
The platinum ring, because it has the lowest specific heat, therefore it requires the least energy to increase the temperature of the ring by 1°C.
The titanium ring, because it has the highest specific heat, therefore it requires the most energy to increase the temperature of the ring by 1°C.
30s - Q7
Examine the table:
A 5g ring of each metal was heated with 100J of energy, which of the four metal rings will have the least temperature change?
The titanium ring, because it has the highest specific heat, therefore it requires the most energy to increase the temperature of the ring by 1°C.
The titanium ring, because it has the highest specific heat, therefore it requires the least energy to increase the temperature of the ring by 1°C.
The platinum ring, because it has the lowest specific heat, therefore it requires the least energy to increase the temperature of the ring by 1°C.
The tin ring, because it has the lowest specific heat, therefore it requires the least energy to increase the temperature of the ring by 1°C.
30s - Q8
Examine the image below: what type of reaction does the energy profile diagram represent? (read the options very carefully)
An exothermic reaction because the energy of products is lower than the energy of the reactants therefore, ΔH is negative and energy is released.
An endothermic reaction because the energy of products is lower than the energy of the reactants therefore, ΔH is positive and energy is absorbed.
An endothermic reaction because the energy of products is lower than the energy of the reactants therefore, ΔH is positive and energy is released.
An exothermic reaction because the energy of products is lower than the energy of the reactants therefore, ΔH is negative and energy is absorbed.
30s - Q9
Examine the image below: what type of reaction does the energy profile diagram represent? (read the options very carefully)
An endothermic reaction because the energy of products is higher than the energy of the reactants therefore, ΔH is positive and energy is absorbed.
An exothermic reaction because the energy of products is lower than the energy of the reactants therefore, ΔH is negative and energy is released.
An exothermic reaction because the energy of products is higher than the energy of the reactants therefore, ΔH is negative and energy is released.
An endothermic reaction because the energy of products is lower than the energy of the reactants therefore, ΔH is positive and energy is released.
30s - Q10
How much heat is needed to raise the temperature of 1000 g of lead from 15.0°C to 25.0°C? (clead= 0.129 J/g°C)
80.75 J
770.52 J
129 J
1290 J
30s - Q11
What mass of barium would have its temperature raised from 65.0˚C to 85.0˚C with the addition of 1000J of heat? (cbarium= 0.201J/g˚C)
0.0995 g
2010 g
248 g
10.05 g
30s - Q12
When 185J of energy is added to 125 g of a silicon sample at 45.0 °C, the temperature increases to 55.0°C. What is the specific heat of the silicon sample?
0.148 J/g°C
2312 J/g°C
6.75 J/g°C
1.48 J/g°C
30s - Q13
How much heat is needed to raise the temperature of 200 g of zinc from 35.0°C to 45.0°C? (czinc= 0.388 J/g°C)
77.6 j
0.0194 J
776 J
5155J
30s - Q14
How much heat is needed to raise the temperature of 118 g of octane from 67.0°C to 87.0°C? (coctane=2.22 J/g°C)
5239 J
2.65 J
0.0763 J
0.376 J
30s - Q15
What mass of titanium would have its temperature raised from 10.8˚C to 20.8˚C with the addition of 1000J of heat? (c Ti= 0.544 J/g˚C)
184 g
544 g
54.4 g
5440 g
30s
