The new temperature is 337.21 K when the pressure was reduced to 101.3 kPa from 150.2 kPa at 500 K.
Explanation:
Data given:
volume of the container = 100 ml
initial pressure on the container P1 = 150.2 kPa
Initial temperature of the container, T1 = 500 K
final temperature of the container, T2 = ?
Final pressure on the container P2 = 101.3 kPa
from the data provided, we will use Gay Lussac's law to calculate the final temperature:
rearranging the equation,
T2 =
Putting the values in the equation:
T2 =
T2 = 337.21 K
thus, the final temperature of the container is 337.21 K
Answer:
A. [isocitrate]/[citrate] = 0.724
B. [citrate] = 24.1 mM
Explanation:
Using the equation, ∆G'° = -RTlnK'eq
Where, ∆G'° = 0.8 KJ/mol = 800 J/mol; R is molar gas constant = 8.315 J/mol; T is standard temperature = 298 K; Keq is equilibrium constant = [isocitrate]/[citrate]
Making Keq subject of formula in the above equation;
Keq = e^(-∆G'°/RT)
= e^ {-800/(8.315*298)}
= e^(-0.323)
Keq = 0.724
Therefore, [isocitrate]/[citrate] = 0.
724
B. Keq = [isocitrate]/[citrate]
Where Keq = 0.724, [isocitrate] = 0.03mM.
[citrate] = Keq/[isocitrate]
= 0.724/0.03
[citrate] = 24.1 mM
Well, figures for efficiency vary a lot, but according to Bicycling Science it’s lubrication that matters most – lubing a dry chain can add 5% to the efficiency.
More interestingly (and I hadn’t read this bit in the book before) it varys a lot depending on gear ratio – bottom gear (22-28) is 99% efficient, top gear (42-11) is 88%. That’s a big difference
Answer:
B the system is unaffected
I think the correct answer would be the third option. The reason I2 has a higher melting point than F2 is because I2 possesses a more polarizable electron cloud. I2 contains more electrons than F2 which would result to a stronger intermolecular forces. Having stronger intermoleculer forces would mean more energy is needed to break the bonds so a higher melting point would be observed.