Technically the answer would be a
Answer:
It corresponds to Charles' Law
Explanation:
Charles's Law corresponds to one of the gas laws, where temperature and volume are related, to constant pressure. That is, according to said equation, the volume of a gas varies directly with the temperature, under conditions of constant pressure.
Answer:
a=28600J; b=90.6 J/K; c=402 torr
Explanation:
(a) considering the data given
Vapour pressure P1 =0 at Temperature T1 = 42.43˚C,
Vapour pressure P2 = 273.15 at Temperature T2= 315.58 K)
Using the Clausius-Clapeyron Equation
ln (P2/P1) = (ΔH/R)(1/T2 - 1/T1)
In 760/140 = ΔH/8.314 J/mol/K × (1/315.58K -- 1/273.15K)
ΔH vap= +28.6 kJ/mol or 28600J
(b) using the Equation ΔG°=ΔH° - TΔS to solve forΔS.
Since ΔG at boiling point is zero,
ΔS =(ΔH°vap/Τb)
ΔS = 28600 J/315.58 K
= 90.6 J/K
(c) using ln (P2/P1) = (ΔH/R)(1/T2 - 1/T1)
ln P298 K/1 atm = 28600 J/8.314 J/mol/K × (1/298.15K - 1/315.58K)
P298 K = 0.529 atm
= 402 torr
Explanation:
N2O4(g) <----------> 2NO2(g)
Before proceeding,
A chemical equilibrium can be defined as a condition in the course of a reversible chemical reaction in which no net change in the amounts of reactants and products occurs.
Statement 1.
This statement is false. Equilibrium is not about equal concentrations but rather zero change in concentration of the reactants and products.
Statement 2.
This statement is True in chemical equilibrium; the forward and reverse reactions occur at equal rates.
Statement 3.
This statement is False. The rate constant for the forward reaction is not equal to the rate constant of the reverse reaction.
Statement 4.
The concentration of NO2 divided by the concentration of N2O4 is NOT equal to a constant. To obtain a constant value irregardless of the concentrations, the concentration of NO2 must be squared. This comes from the stoichiometry of the reaction
Kc= [NO2]2 / [N2O4]
This statement is false.
