The answer is A, good luck
Answer:
Approximately , assuming that this acid is monoprotic.
Explanation:
Assume that this acid is monoprotic. Let denote this acid.
.
Initial concentration of without any dissociation:
.
After of that was dissociated, the concentration of both and (conjugate base of this acid) would become:
.
Concentration of in the solution after dissociation:
.
Let , , and denote the concentration (in or ) of the corresponding species at equilibrium. Calculate the acid dissociation constant for , under the assumption that this acid is monoprotic:
.
Answer:
0.2g
Explanation:
All radiodecay follows the 1st order decay equation
A = A₀e^-kt
A => Activity at time (t)
A₀ => Initial Activity at time = 0
k => decay constant for isotope
T => time in units that match the decay constant
Half-Life Equation => kt(½) = 0.693 => k = 0.693/34 min = 0.0204min¹
A = A₀e^-kt = (26g)e^-(0.0204/min)(238min) = (26g)(0.0078) = 0.203g ~ 0.2g (1 sig fig).
The energy containing electron transporters of FADH2 are not produced during glycolysis.
Answer:
4.78atm
Explanation:
From the question, we obtained the following:
P1 (initial pressure) = 3.5 atm
T1 (initial temperature) = 200K
T2 (final temperature) = 273K
P2 (final pressure) =?
Using P1/T1 = P2/T2, the final pressure can be obtained as shown below:
P1/T1 = P2/T2
3.5/200 = P2/273
Cross multiply to express in linear form as shown below:
200 x P2 = 3.5 x 273
Divide both side by 200
P2 = (3.5 x 273)/200
P2 = 4.78atm
Therefore, the pressure at 273K is 4.78atm