3.2.1 Enthalpy changes Flashcards
including measuring enthalpy changes spec. ref. = 3.2.1, 2.1.3 and Hess's Law and enthalpy cycle questions spec. ref. = 3.2.1
what happens in an exothermic reaction
energy is released causing the temperature of the surroundings to increase
describe the enthalpy change profile of an exothermic reaction
Energy is released
SO products are lower in energy than reactants
SO enthalpy change (𝚫H) is negative
What happens in an endothermic reaction
Energy is absorbed causing the temperature of the surroundings to decrease
Describe the enthalpy change profile of an endothermic reaction
Energy is absorbed
SO products are higher in energy than reactants
SO enthalpy change (𝚫H) is positive
desribe the enthalpy change (𝚫H) arrow on an enthalpy profile
The arrow goes from the reactants to the products it will be up for endothermic (+ve) reactions and pointing down for exothermic reactions (-ve)
what is activation energy (Ea)
Activation energy is the minimum amount of energy required to start a reaction (by breaking bonds)
Describe the activation energy (Ea) arrow on an enthalpy profile
The arrow always goes up. it goes from the same level as the reactants to the top of the arch (therefore needing to be in the middle NOT on the reactant line)
What 2 equations are used to calculate 𝚫H
and in what order
Q = mc𝚫T
then 𝚫H = Q/n
energy = mass of water x specific heat capacity x the change in temperature
enthalpy change = energy divided by number of moles
what are the units for Q = mc𝚫T
Joules = grams x (J/g/℃) x ℃
what
what are the units for 𝚫H = Q/n
(KJ/mol) = joules x number of moles
what is the equation for 𝚫H using the enthalpy of the products and reactants
𝚫H = H(products) - H(reactants)
what is the law of the conservation of energy
energy cannot be created or destroyed
what is this symbol for 𝚫H⦵
the ⦵ should be smaller and in the top right (superscript)
standard enthalpy change
takes place under standard conditions
what are standard conditions
- components in their standard states
- standard conditions:
298K
1atm (101kpa)
1moldm⁻³
what is 𝚫H⦵r for
the r would normally be in the bottom right (subscript)
standard enthaply change of reaction
define standard enthalpy change of reaction
enthalpy change that accompanies a reaction in the molar quantities shown
what is 𝚫H⦵c for
the c would normally be in the bottom right (subscript)
standard enthaply change of combustion
define standard enthalpy change of combustion
enthalpy change when 1 mol of a substance completely reacts with O₂
what is 𝚫H⦵f for
the f would normally be in the bottom right (subscript)
standard enthalpy change of formation
define standard enthalpy change of formation
enthalpy change when 1 mol of a substance is formed from its elements in their standard states
what is 𝚫H⦵neut
the neut would normally be in subscript
standard enthalpy change of neutralisation
define standard enthalpy change of neutralisation
enthalpy change when an acid and a base react to form 1 mol of water
state Hess’s Law
The enthalpy change of any 2 route is the same as long as the initial and final states are the same
what does Hess’s Law do
Hess’s law provides a way of measuring 𝚫H indirectly
why can some 𝚫H not be measured directly
- they have a very high Ea
- the reaction is very slow
- there are a mixture of side reactions or products
How do you calculate 𝚫H using 𝚫Hf data
𝚫H of say reaction - not that important to the question
𝚫Hr = - 𝚫Hf(reactants) + 𝚫Hf(products)
OR
𝚫Hr = 𝚫Hf(products) - 𝚫Hf(reactants)
they are the same just different ways around
How do you calculate 𝚫H using 𝚫Hc data
𝚫Hr = 𝚫Hc(reactants) - 𝚫Hc(products)
how do you convert from kelvin to ℃
add 273 to the ℃
using a spirit burner
describe an experiment that gives 𝚫Hc data
liquid fuels such as methanol can be burned easily using a small spirit burner.
1. Using a measuring cylinder, measure out 150cm³ of water. pour the water into the beaker and record the initial temperature of the water ( to the nearest 0.5℃)
2. Add methanol to the spirit burner. weigh this and record the mass.
3. place the spirit burner under the beaker, and light it whilst stiring the water with a thermometer.
4. after ~3mins extinguish the flame. Immediately record the maximum temperature reached by the water
5. reweigh the spirit burner with methanol in and assume the wick has not been burned
As the water has gained energy the methanol must have lost the same amount of energy so the 𝚫H is negative and the reaction exothermic - keep in mind for Q calculation and then the 𝚫H calculation use this symbol at the end to check
why may experimental 𝚫Hc data be inaccurate
- there is heat loss to the surroundings other than water (this includes the beaker but maining the air surrounding the flame)
- incomplete combustion of methanol
- evapouration of methanol from the wick ( the burner must be weighed immediately after extinguishing the flame, otherwise some methanol my evapourate - spirit burners usually have a cover to minimise this)
- Non-standard conditions