39 J
P=Fd/t i belive is the answer
Answer:
4.39
Explanation:
Let's consider the following reaction at equilibrium.
2 NH₃(g) ⇄ 3 H₂(g) + N₂(g)
The concentration equilibrium constant (Kc) is the product of the concentration of the products raised to their stoichiometric coefficients divided by the product of the concentration of the reactants raised to their stoichiometric coefficients.
Kc = [H₂]³.[N₂]/[NH₃]²
Kc = (0.700)³.(0.800)/(0.250)²
Kc = 4.39
Explanation:
The answer is
153.7
k
J
.
What you are asked to determine is the total energy required to go from ice to water, and then from water to vapor - the phase changes underwent by the water molecules.
In order to do this, you'll need to know:
Heat of fusion of water:
Δ
H
f
=
334
J
/
g
;
Heat of fusion vaporization of water:
Δ
H
v
=
2257
J
/
g
;
Specific heat of ice:
c
=
2.09
J
/
g
∘
C
;
Specific heat of water:
c
=
4.18
J
/
g
∘
C
;
Specific heat of steam:
c
=
2.09
J
/
g
∘
C
;
So, the following steps describe the overall process:
1. Determine the heat required to raise the temperature of the ice from
−
15.0
∘
C
to
0
∘
C
:
q
1
=
m
⋅
c
i
c
e
⋅
Δ
T
=
50.0
g
⋅
2.09
J
g
⋅
∘
C
⋅
(
0
∘
C
−
(
−
15
∘
C
)
)
=
1567.5
J
2. Determine the heat required to convert
0
∘
C
ice to
0
∘
C
water:
q
2
=
m
⋅
Δ
H
f
=
50.0
g
⋅
334
J
g
=
16700
J
3. Determine the heat required to go from water at
0
∘
C
to water at
100
∘
C
:
A substance where almost all have the same atomic number of protons
Solvent is used to dissolve the solute in the solution