WorksheetsTopic 5 Thermo
Total questions: 10
Worksheet time: 5mins
What is shown by the reaction 2C(s) + 3H2 (g)+21O2 (g)→ C2 H5 OH (l)
Enthalpy of Combustion
Enthalpy of Formation
Bond enthalpy
Lattice Enthalpy
When barium hydroxide and ammonium thiocyanate are mixed the temperature drops. Which statement is true?
The reaction is __________ and Δ H is ________
endothermic, negative
endothermic, positive
exothermic, negative
exothermic, positive
Energy is ____ when bonds are formed and ____ when they are broken.
absorbed, absorbed
released, released
absorbed, released
released, absorbed
The temperature of a 2.0 g sample of aluminum increases from 25 C to 30C. How many joules of heat energy were added? (Specific heat of Al = 0.90 J/gK)
0.36
2.3
9.0
11
The temperature in Kelvin of 1.0 dm3 of an ideal gas is doubled and its pressure is tripled. What is the final volume of the gas is
1/3
2/3
3/2
1/6
Given the following specific heat capacities, which metal will show the greatest increase in temperature if 50 J is added to 1 g of metal?
Cu 385 Ag 234 Au 130 Pt 134
Cu
Ag
Au
Pt
A reaction is exothermic,
Products are more stable than reactants
Reactants are more stable than products
Delta H is positive
Ea is negative
The reaction shown is
endothermic
exothermic
isothermic
don't pick me
Which reaction is endothermic?
burning gasoline
neutralization of HCl with NaOH
photosynthesis
sodium in water
Which of the following statements are true for the reaction:
SO2(g) + 1/2O2(g) ↔ SO3(g)
ΔH = –92 kJ mol-1
Where ↔ indicates that the reaction can proceed in the forward and the reverse direction.
The forward and reverse reaction both produce 92 kJ of energy.
Oxidizing 2 moles of SO2 would produce twice as much energy.
The reverse reaction has an enthalpy of 1/-92kJ mol-1.
Collecting the SO3 produced in the liquid state would not change the measured enthalpy.
