Thermochemistry Test 6a2046
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TUITION TEST:: CLASS XI:: CHEMISTRY:: THERMODYNAMICS Full Marks: 20
Time: 10 min.
A. Write the equations: 1.
1X 2=2
∆H vs. ∆E; Change in enthalpy is equal to the sum of change in energy and the product of the change in the number of moles of gas and RT where R = 8.31 J/mol K and and T is in kelvin
2.
First law of thermodynamics; Total change in energy equal to the sum of work and heat flow
B. Choose the correct option 1.
1X 5=5
Heat flow; Where m = mass, c = specific heat, and ∆t = change in temperature (final - initial) 1.
q = C x ∆t
2.
∆E = q + w
3.
∆H = ∆E + ∆ngRT
4.
q = m x c x ∆t
b. Bomb calorimeter: This can be used to find the amt of heat absorbed/evolved in a reaction if you know the heat capacity (C cal), and ∆t = change in temperature 1.
q = m x c x ∆t 2.
q = C x ∆t
3.
q reaction = -q calorimeter
TUITION TEST:: CLASS XI:: CHEMISTRY:: THERMODYNAMICS 4.
q reaction = -C cal x ∆t
b. Where C = heat capacity(J/ºC), and ∆t = the change in temperature (final initial) 1.
∆H = qv 2.
q = m x c x ∆t
3.
∆H = qp
4.
q = C x ∆t
b. 4.18 J/gºC 1.
q = C x ∆t 2.
q = m x c x ∆t
3.
Specific Heat of H₂O
4.
∆H = qp
b. Change in enthalpy is equal to the sum of change in energy and the change in the product of PV 1.
∆E = q + w 2.
∆H = ∆E + ∆(PV)
TUITION TEST:: CLASS XI:: CHEMISTRY:: THERMODYNAMICS 3.
∆H = ∆E + ∆ngRT
4.
∆H = ∆H₁ + ∆H₂
C. State true or false 1X4=4 1.
q reaction = -C cal x ∆t → Represents how the heat flow for the reaction system is equal in magnitude but opp in sign to that of the calorimeter True
2.
∆E system = -∆E surroundings → Law of conservation of energy True
3.
False
False
∆H = ∆E + ∆ngRT → Change in enthalpy is equal to the sum of change in energy and the change in the product of PV True
4.
False
∆H = ∆H₁ + ∆H₂ → Change in enthalpy is equal to the sum of change in energy and the change in the product of PV True
False
D. Write equations 1. Standard enthalpy change; Finding the enthalpy of formation
1X4=4
TUITION TEST:: CLASS XI:: CHEMISTRY:: THERMODYNAMICS 2. Where C = heat capacity(J/ºC), and ∆t = the change in temperature (final initial)
3. Heat flow; Where m = mass, c = specific heat, and ∆t = change in temperature (final - initial)
4. Difference in enthalpy is equal to the heat flow for the reaction system
E. Multiple choice questions 1.
1X5=5
Heat flow at constant pressure is equal to change in enthalpy 1.
∆H = qv
2.
q = C x ∆t
3.
∆H = qp
4.
∆E = q + w
b. First law of thermodynamics; Total change in energy equal to the sum of work and heat flow 1.
∆E = q + w 2.
q = C x ∆t
3.
∆H = qv
4.
∆H = qp
TUITION TEST:: CLASS XI:: CHEMISTRY:: THERMODYNAMICS b. Represents how the heat flow for the reaction system is equal in magnitude but opposite in sign to that of the calorimeter 1.
q reaction = -q calorimeter 2.
q reaction = -C cal x ∆t
3.
q = m x c x ∆t
4.
∆E = q + w
b. Heat flow at constant volume is equal to change in enthalpy 1.
q = C x ∆t 2.
∆E = q + w
3.
∆H = qp
4.
∆H = qv
b. Change in enthalpy is equal to the sum of change in energy and the change in the product of PV 1.
∆E = q + w 2.
∆H = ∆E + ∆ngRT
3.
∆H = ∆H₁ + ∆H₂
4.
∆H = ∆E + ∆(PV)
Time: 10 min.
A. Write the equations: 1.
1X 2=2
∆H vs. ∆E; Change in enthalpy is equal to the sum of change in energy and the product of the change in the number of moles of gas and RT where R = 8.31 J/mol K and and T is in kelvin
2.
First law of thermodynamics; Total change in energy equal to the sum of work and heat flow
B. Choose the correct option 1.
1X 5=5
Heat flow; Where m = mass, c = specific heat, and ∆t = change in temperature (final - initial) 1.
q = C x ∆t
2.
∆E = q + w
3.
∆H = ∆E + ∆ngRT
4.
q = m x c x ∆t
b. Bomb calorimeter: This can be used to find the amt of heat absorbed/evolved in a reaction if you know the heat capacity (C cal), and ∆t = change in temperature 1.
q = m x c x ∆t 2.
q = C x ∆t
3.
q reaction = -q calorimeter
TUITION TEST:: CLASS XI:: CHEMISTRY:: THERMODYNAMICS 4.
q reaction = -C cal x ∆t
b. Where C = heat capacity(J/ºC), and ∆t = the change in temperature (final initial) 1.
∆H = qv 2.
q = m x c x ∆t
3.
∆H = qp
4.
q = C x ∆t
b. 4.18 J/gºC 1.
q = C x ∆t 2.
q = m x c x ∆t
3.
Specific Heat of H₂O
4.
∆H = qp
b. Change in enthalpy is equal to the sum of change in energy and the change in the product of PV 1.
∆E = q + w 2.
∆H = ∆E + ∆(PV)
TUITION TEST:: CLASS XI:: CHEMISTRY:: THERMODYNAMICS 3.
∆H = ∆E + ∆ngRT
4.
∆H = ∆H₁ + ∆H₂
C. State true or false 1X4=4 1.
q reaction = -C cal x ∆t → Represents how the heat flow for the reaction system is equal in magnitude but opp in sign to that of the calorimeter True
2.
∆E system = -∆E surroundings → Law of conservation of energy True
3.
False
False
∆H = ∆E + ∆ngRT → Change in enthalpy is equal to the sum of change in energy and the change in the product of PV True
4.
False
∆H = ∆H₁ + ∆H₂ → Change in enthalpy is equal to the sum of change in energy and the change in the product of PV True
False
D. Write equations 1. Standard enthalpy change; Finding the enthalpy of formation
1X4=4
TUITION TEST:: CLASS XI:: CHEMISTRY:: THERMODYNAMICS 2. Where C = heat capacity(J/ºC), and ∆t = the change in temperature (final initial)
3. Heat flow; Where m = mass, c = specific heat, and ∆t = change in temperature (final - initial)
4. Difference in enthalpy is equal to the heat flow for the reaction system
E. Multiple choice questions 1.
1X5=5
Heat flow at constant pressure is equal to change in enthalpy 1.
∆H = qv
2.
q = C x ∆t
3.
∆H = qp
4.
∆E = q + w
b. First law of thermodynamics; Total change in energy equal to the sum of work and heat flow 1.
∆E = q + w 2.
q = C x ∆t
3.
∆H = qv
4.
∆H = qp
TUITION TEST:: CLASS XI:: CHEMISTRY:: THERMODYNAMICS b. Represents how the heat flow for the reaction system is equal in magnitude but opposite in sign to that of the calorimeter 1.
q reaction = -q calorimeter 2.
q reaction = -C cal x ∆t
3.
q = m x c x ∆t
4.
∆E = q + w
b. Heat flow at constant volume is equal to change in enthalpy 1.
q = C x ∆t 2.
∆E = q + w
3.
∆H = qp
4.
∆H = qv
b. Change in enthalpy is equal to the sum of change in energy and the change in the product of PV 1.
∆E = q + w 2.
∆H = ∆E + ∆ngRT
3.
∆H = ∆H₁ + ∆H₂
4.
∆H = ∆E + ∆(PV)
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