Answer:
The molar heat capacity at constant volume is 21.62 JK⁻¹mol⁻¹
The molar heat capacity at constant pressure is 29.93 JK⁻¹mol⁻¹
Explanation:
We can calculate the molar heat capacity at constant pressure from
Where 
is the molar heat capacity at constant pressure
is the heat capacity at constant pressure
and 
is the number of moles
Also is given by
Hence,
becomes
From the question,
= 229.0 J
= 3.00 mol
= 2.55 K
Hence,
becomes
29.93 JK⁻¹mol⁻¹
This is the molar heat capacity at constant pressure
For, the molar heat capacity at constant volume,
From the formula
Where 
is the molar heat capacity at constant volume
and 
is the gas constant ( = 8.314 JK⁻¹mol⁻¹)
Then,
21.62 JK⁻¹mol⁻¹
This is the molar heat capacity at constant volume
Answer:
- 20 J
Explanation:
Heat of Reaction = Heat of Products - Heat of Reactants
From the graph;
Heat of Products = 10
Heat of Reactants = 30
Heat of Reaction = 10 - 30 = -20 J
You can reduce the charges and subscripts so it is PbS2
Answer:
0.272 mol
Explanation:
∆Tb = m × Kb
∆Tb = 85.2°C - 78.4°C = 6.8°C
Kb = 1.22°C/m
mass of ethanol = 48.80 g = 48.80/1000 = 0.0488 kg
Let the moles of non-ionizing solute be y
m (molality) = y/0.0488
6.8 = y/0.0488 × 1.22
y = 6.8×0.0488/1.22 = 0.272 mol
