Thermodynamics Study Guide
It's value represents the change in randomness as a reaction proceeds.
Entropy, often described as randomness in a system, is subject to change in any chemical reaction. The value for ΔS can be (+ or -). Answer: ΔS
A cube of ice is added to some hot water in an insulated container which is then sealed. There is no heat exchange with the surroundings. Which describes the system once it has shifted to a new equilibrium? 1. The average kinetic energy of the liquid phase has decreased 2. The total energy of the system has decreased. 3. The entropy of the system has increased.
1, and 3 only
Which applies to any reaction that has negative values for both ΔH and ΔS? 1. The reaction is spontaneous at all temperatures 2. The reaction is exothermic 3. ΔG increases (becomes more positive) as temperature increases.
2, and 3 only
The heat of neutralization for a strong acid in dilute water solution is about 60 kJ mol-1. What quantity of heat in kJ is produced when 100. mL of 1.0 M H2SO4 is mixed with 100. mL of 1.0 M KOH?
6.0
The molar heat of fusion, ΔH fus, for water is 6.01 kJ mol -1. Which expression gives the molar heat entropy of fusion, ΔS fus, in kJ -1 mol -1 for ice at its normal melting point?
6.01/273
The molar heat of fusion, ΔH fus, for water is 6.01 kJ mol -1. The specific heat capacity for water, Cp, is 75 J mol-1 deg. C -1. Which expression gives the quantity of energy needed to change 1.0 mol ice at 0 deg Celcius to liquid water at 25 deg Celsius?
6010 + (75 X 25)
It's value is determined by using molar concentrations at equilibrium in the mass action expression.
The equilibrium constant is determined by the molar concentration of reactants and products at equilibrium in a closed system according to the formula. Products/Reactants. Answer: Kc
It's value is calculated using the absolute (Kelvin) temperature and 2 of the other choices from the set.
ΔG
It's value is negative for any spontaneous reaction.
ΔG
The change in enthalpy is negative for any exothermic reaction.
ΔH
