Thermochemistry
These are the two types of reactions related to heat.
What are Endothermic and Exothermic?
This is the amount of heat released or absorbed during the phase change of 1 mole of a material.
What is molar enthalpy?
A way to measure heat change in a chem/physical process.
What is calorimetry?
This is the standard state of oxygen.
What is O2?
The measure of disorder or randomness of the particles that make up a system.
What is entropy?
This is the equation for thermochemistry
What is Q = MCp∆T?
∆H equals (equation).
What is Hproducts - Hreactants ?
This type of reaction has the same amount of heat in the system as the surrounding.
What is an endothermic reaction?
This is the ∆H of every free element in its standard state.
What is 0.0kJ?
Spontaneous processes always proceed in such a way that the entropy of the universe increases.
What is the law of disorder?
Joules of energy released by a 143 Calorie granola bar. (1 Calorie = 4186 J)
What is 598, 598 J (598.598 kJ)
Since you cannot actually measure enthalpy, this is measured instead.
What is heat absorbed or released in a chemical reaction?
The amount of heat it takes to raise the temperature of 1 gram of a substance by 1˚C.
What is specific heat capacity
(Cp )?
This is the change in enthalpy that accompanies the formation of one mole of a compound in its standard start from its constituent elements in their standard states
What is standard enthalpy?
The G in ∆G˚ system = ∆H˚ system - T∆S˚system stands for this.
What is Gibbs's free energy (available to do work)?
This is the amount of heat that it takes to raise 1 gram of a substance by 1°C
What is a calorie?
This is the ∆H for this equation.
2S(s) + 3O2(g) → 2SO3 (g) ∆H = ?
a) S(s) + O2(g) → SO3(g) ∆H = -297kJ
b) 2SO3(g) → 2SO2(g) + O2(g) ∆H = 198kJ
What is ∆H = -792kJ?
If 40.5 J of heat is added to a 15.4 g of silver, this is how much the temperature will increase by. The specific heat of silver is 0.235 J/(g°C).
What is 11.191°C?
This is the ∆H for the following reaction. (∆Hf = ∆H(products) - ∆H(reactants))
CH4(∆H =-74.9) + 2O2(∆H =0) → CO2(∆H =-393.5) + 2H2O(∆H =-285.8)
What is ∆H = -890.2 kJ?
When ∆H and ∆S are both positive, name the chance of spontaneity.
What is spontaneous only with a high temp?
The temperature of a piece of copper with a mass of .0954 kg changes from 25° C to 48° C when metal absorbs 849 J of heat. Find the specific heat. (Cp)
What is 0.387 J/gC°?
How much heat is evolved when 54g glucose (C6H12O6) (Molar Mass = 180g/mol) is burned according to the following equation? (∆H = -2808kJ/mol)
C6H12O6(s) + 12O2(g) → 6CO2(g) + 6H2O(l)
What is -824.4 kJ released?
A 28.4 g sample of aluminum is heated to 39.4°C, then placed in a calorimeter containing 50.0 g of water. The temperature of water increases from 21.00°C to 23.00°C. The specific heat of aluminum.
What is 0.897 J/(g°C)?
This is the ∆H for the following reaction, (∆Hf = ∆H(products) - ∆H(reactants))
H2S(∆H =-20.6) + 4F2(∆H =0) → 2HF(∆H =-273.3) + SF6(∆H =-1209)
What is ∆H = -1735 kJ?
G = Spontaneous or non spontaneous:
∆H = 27.6 kJ
T = 535 K
∆S = -55.2 J/K
What is ∆G = +1932 J so non-spontaneous?