We have to know final temperature of the gas after it has done 2.40 X 10³ Joule of work.
The final temperature is: 75.11 °C.
The work done at constant pressure, W=nR(T₂-T₁)
n= number of moles of gases=6 (Given), R=Molar gas constant, T₂= Final temperature in Kelvin, T₁= Initial temperature in Kelvin =27°C or 300 K (Given).
W=2.4 × 10³ Joule (Given)
From the expression,
(T₂-T₁)=
(T₂-T₁)=
(T₂-T₁)= 48.11
T₂=300+48.11=348.11 K= 75.11 °C
Final temperature is 75.11 °C.
Answer:
The volume will be 2600 L.
Explanation:
Initial temperature () = 25°C = (25 + 273) K = 298K
Final temperature () = 54°C = (54 + 273) K = 327 K
By using the combined gas law equation,
=
or, =
or, 3060 × 327 = 380 ×
or, ≈ 2600 L
Hence the volume of the balloon will be about 2600 L.
Explanation:
A chemical equilibrium is defined as the state of reaction in which the rate of forward reaction is equal to the rate of backward reaction.
When Q > , then it means that the reaction is proceeding in the backward reaction. Whereas if Q <
, then it means that the reaction is proceeding in the forward direction. Hence, formation of products will be favored.
On the other hand, if Q = , then it means reaction is at equilibrium.
At equilibrium, it is not necessary that the concentrations of products divided by the concentrations of reactants equals one.
Thus, we can conclude that the statement for a chemical system at equilibrium, the forward and reverse rates of reaction are equal, is correct.