I JATW THAT I NEED TO ANSWER TO ASK
Answer: E=∆H*n= -40.6kj
Explanation:
V(CO) =15L=0.015M³
P=11200Pa
T=85C=358.15K
PV=nRT
n=(112000×0.015)/(8.314×358.15)
n(Co)= 0.564mol
V(Co)= 18.5L = 0.0185m³
P=744torr=98191.84Pa
T= 75C = 388.15k
PV=nRT
n= (99191.84×0.0185)/(8.314×348.15)
n(H2) = 0.634mol
n(CH30H) =1/2n(H2)=1/2×0.634mol
=0.317mol
∆H =∆Hf{CH3OH}-∆Hf(Co)
∆H=-238.6-(-110.5)
∆H = 128.1kj
E=∆H×n=-40.6kj.
Answer:
D. 18,800 J/mol
Explanation:
We need to use the Arrhenius equation to solve for this problem:
, where k is the rate constant, A is the frequency factor, 
is the activation energy, R is the gas constant, and T is the temperature in Kelvins.
We want to find the value of , so let's plug some of the information we have into the equation. The gas constant we can use here is 8.31 J/mol-K.
At 0°C, which is 0 + 273 = 273 Kelvins, the rate constant k is 
. So:
At 20°C, which is 20 + 273 = 293 Kelvins, the rate constant k is 
. So:
We now have two equations and two variables to solve for. We just want to find Ea, so let's write the first equation for A in terms of Ea:
Plug this in for A in the second equation:
After some troublesome manipulation, the answer should come down to be approximately:
Ea = 18,800 J/mol
The answer is thus D.
Answer:
Increased surface area - finely divided solute
like dissolves like - matching polarity
temperature - rate proportional to kinetic energy
stirring spreads - solute throughout solution
