measure of the disorder or randomness of the particles that make up a system
What is entropy?
100
This means the reaction is nonspontaeous
What is a positive delta G
100
Is this spontaneous?
deltaH= -75.9kJ
T=273 K
deltaS= 138 J/K
What is yes
100
S
What is entropy?
100
type of reaction that gets cold
What is endothermic reaction?
200
the heat content of a system at constant pressure
What is enthalpy
200
delta G is negative
What is a spontaneous reaction
200
Is this spontaneous?
deltaH= -27.6kJ
T=535 K
deltaS= -55.2 J/K
What is no
200
ΔH
What is change in enthalpy
200
type of reaction that gets hot
What is exothermic?
300
energy that is available to do work
What is Gibbs free energy
300
delta H is positive and TdeltaS is negative
What is nonspontaneous
300
Is this spontaneous and what is deltaG?
deltaH= 635kJ
T=388 K
deltaS= -55.2 J/K
What is no, 386,000
300
ΔG
What is free energy change?
300
The definiton of spontaneous process
What is a physical or chemical change that occurs with no outside intervention?
400
A greater amount of energy is required to break bonds than to form new bonds
What is an endothermic reaction
400
Conditions that make a reaction always be spontaneous
What is negative deltaH and a positive TdeltaS
400
The standard free energy change ΔG for the following reaction at 25oC?
N2 + 3H2 → 2NH3
The values for ΔH ang S is -91.8KJ and -198.0J/K
What is ΔG = -32.8KJ
400
T (what units)
What is temperature in Kelvin?
400
The sign ΔG would have been in the video for the reaction
What is positive?
500
a greater amount of energy is released than is required to break bonds in initial reaction
What is an exothermic reaction?
500
Spontaneous if the absolute value of ΔH is greater than the absolute value of TΔS
What is negative for both deltaH and TdeltaS?
500
The standard Gibbs free energy change for the formation of methane from carbon and hydrogen at 298K.
Given the ΔH value is -74.9KJ/mol ΔS = -80.7J/K.mol
What is ΔG = -50.9KJ/mole
500
ΔH(degree sign)
What is change in enthalpy at standard conditions?