Unit 2.1 Thermochemistry Flashcards
(20 cards)
Well it states to acknowledge the principle of conservation of energy (literally physics)
Energy cannot be destroyed or created only transferred from one form to another
2 examples of an endothermic reaction?
- Photosynthesis
- Decomposition of CaCO3
3 examples of an exothermic reaction?
- Respiration
- Combustion
- Metal + acid
I shall hope u already know how to create reaction profiles for exothermic and endothermic reactions
(either refer to book or the next unit)
worth it?
saves time.
meh
If endothermic, △H = ?
Positive
If exothermic, △H = ?
Negative
In terms of △H, what makes the products of a chemical reaction more stable
More exothermic
More negative
More -△H
Define bond enthalpy
The enthalpy required to break a covalent X-Y bond into X atoms and Y atoms, all in the gas phase
Define average bond enthalpy
The average value of the enthalpy required to break a given type of covalent bond in the molecules of a gaseous species
How to calculate standard enthalpy change
- I assume we are actually given a table of energy for each bond
- Doesn’t matter which side is products or reactants:
- Minus the left side with the right side
- Can determine whether it’s exothermic or endothermic
- What may be difficult:
How to tell what bonds are there within a chemical compound?
Explain standard enthalpy change of formation △Hfθ or △fHθ
The enthalpy change when:
- 1 mole of product is formed
- in standard state under standard conditions
- Changes = negative
- Units = kJmol-1
a) C(s) + ½O2(g) -> CO(g)
b) 2C(s) + O2(g) -> 2CO(g)
c) C(g) + ½O2(g)) -> CO(g)
WHICH of these reactions show standard molar enthalpy of formation. Explain.
a). You know why?:
- 1 mole
- C = solid
- Idk if it actually is negative, whatever u can figure that out
a) H(g) + ½Br2(l) -> HBr(g)
b) H2(g) + Br2(l) -> 2HBr(g)
c) ½H2(g) + ½Br2(l) -> HBr(g)
WHICH OF THESE reactions show standard molar enthalpy of formation. Explain.
c). YOU KNOW why?
- 1 mole again
- Show it’s also H2 right?
but it’s smart cuz u can just write down ½ duhhh
- Could be negative? Nega
Explain standard enthalpy change of combustion △Hcθ or △cHθ
The enthalpy change when:
- 1 mole of a substance
- Completely combusted in oxygen
- Under standard conditions
- Negative kJmol-1
Ethane (C2H6) and carbon (C) as a thermochemical reaction for the standard molar enthalpy of combustion?
ethane (△Hcθ = -1560kJmol-1):
C2H6(g) + 3½O2(g) -> 2CO2(g) + 3H2O(l)
carbon (△Hcθ = -394kJmol-1:
C(s) + O2(g) -> CO2(g)
Ya see how they’re all negative? (exothermic)
Difference of standard molar enthalpy of formation of potassium oxide (K2O) between △Hfθ and △Hcθ
△Hfθ = 2K(s) + ½O2(g) -> K2O(s)
△Hcθ = K(s) + ¼O2(g) -> ½K2O(s)
I think the trick here is:
△Hfθ = 1 mole of product
△Hcθ = 1 mole of substance (reactant perhaps?)
What does the θ mean seen in the notation △Hfθ or △Hcθ?
Theta/plimsoll:
- Under standard conditions
- Temp: 298K, 25°C
- Pressure: 1 atm, 10100pa? [101325pa???]
Explain enthalpy change of reaction △Hr or △rH
The enthalpy change in a reaction between the number of moles shown in the reaction equation
After a long consideration, this is the exact same as finding the bond enthalpy change at the beginning. BUT IF IT’S GONNA STATE THE DIFFERENCE:
- Heat given off or taken up for the reaction
State Hess’s Law
The total enthalpy change for a reaction is independent of the route taken from the reactants to the products
Wait
Wait?