Answer:
All you have to do here is use the ideal gas law equation, which looks like this
P
V
=
n
R
T
−−−−−−−−−−
Here
P
is the pressure of the gas
V
is the volume it occupies
n
is the number of moles of gas present in the sample
R
is the universal gas constant, equal to
0.0821
atm L
mol K
T
is the absolute temperature of the gas
Rearrange the equation to solve for
T
P
V
=
n
R
T
⇒
T
=
P
V
n
R
Before plugging in your values, make sure that the units given to you match those used in the expression of the universal gas constant.
In this case, the volume is given in liters and the pressure in atmospheres, so you're good to go.
Plug in your values to find
T
=
3.10
atm
⋅
64.51
L
9.69
moles
⋅
0.0821
atm
⋅
L
mol
⋅
K
T
=
251 K
−−−−−−−−−
The answer is rounded to three sig figs
Step-by-step explanation:
hope it helps