A container of oxygen with a fixed volume has a pressure of 13.0 atm at a temperature of 20 °C. What will the pressure of the ox ygen be if the container is heated to 102 °C? A. 12.4 atm B. 15.4 atm C. 16.6 atm D. 18.6 atm
1 answer:
Given:
P1 = 13.0 atm
T1 = 20 °C
T2 = 102 °C
Required:
P2 of oxygen
Solution:
At constant volume,
we can apply Gay-Lussac’s law of pressure and temperature relationship
P1/T1=P2/T2
(13.0 atm) / (20 °C)
= P2 / (102 °C)
P2 = 66.3 atm
The answer is not in the choices given.
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There are 4 significant figures(3050)
Explanation:
Given:
20.5 torr
78.6 torr
225 torr
Change into atm
Computation:
We know that;
1 torr = 0.00131579 atm
So,
1. 20.5 torr
= 20.5 x 0.00131579 atm
= 0.02697
= 0.027 atm (Approx)
2. 78.6 torr
= 78.6 x 0.00131579 atm
= 0.103090
= 0.103 atm (Approx)
3. 225 torr
= 225 x 0.00131579 atm
= 0.2960
= 0.296 atm (Approx)
Answer:
D. +5.7 kJ/mol
Explanation:
Molar free energy (ΔG) in the transportation of uncharged molecules as glucse through a cell membrane from the exterior to the interior of the cell is defined as:
ΔG = RT ln C in / C out
knowing R is 8,314472 kJ/molK; T is 298K Cin = 200mM and Cout = 20mM
ΔG = 5,7 kJ/mol
Right answer is:
D. +5.7 kJ/mol
I hope it helps!
Although I’m not entirely sure what answer you’re looking for, I’d say because most scientific investigations require multiple trials of an experiment
