Thermodynamics | Assignment-1

THERMODYNAMICS
By Name
Course
Instructor
Institution
Location
Date
Q1

Heat capacity q = Supplied heat energy
Rise∈temperature
Heat capacity q = 125
310−277
Heat capacity q = 125
33
Heat capacity q =3.7878 kJ/C
The value of q
q= mc∆ T
where m is mass c is specific heat capacity of water , q is heat energy and ∆ T is change in
absolute temperature
q= mc∆ T
q= 0.075× 4.18 ×33
q= 10.3455 kJ/mol
Value of ∆ H
At a constant pressure the formula for q is the same as the formula for ∆ H thus
∆ H =q= mc∆ T and ∆ H = 10.3455 kJ/mol
Q2
i.
From Q= nC∆ T
Where n is the number of moles, Q is the heat flow, C is the molar heat capacity and ∆ T is the
temperature change.
Moles 54000
18 = 3000 moles

3000×75 × ∆ T = 7000000
225000 ∆ T
225000 = 7000000
225000
∆ T = 31.1 K
ii.
When there is no change in temperature
0
mC ∆ T +m ∆ vapH =7000000
m× 44000
44000 = 7000000
44000
m= 159.09g
Q3
Molar capacity at constant pressure C p ,m
∆ H =q= C p ,m ∆ T
Where C is the heat capacity ∆ T change in temperature
∆ H =38.5×(310−277)
∆ H = 1270.5 J/K
Q4
a)
Um =
Hm + TS ( FALSE )
b) b)
Hm =
Um – RT (FALSE)
c) c)
Hm =
Um + RT ( TRUE)
d) d)
Um =
Hm / TS ( TRUE)
Q5
∆ S0=∑
n
n S0 ( products )−∑
m
m S0 (reactants)
∆ S0 = {(1mole×129.2 ¿+(1 mole ×111)}- {(1mole×213.4 ¿+(1 mole × 69.9)}
∆ S0 = 240- 273.3