What is the pressure of 0.540 mol of an ideal gas at 35.5 l and 223k use pv=nrt and r=8.314 l•kpa/mol•k

0.278 atm

Explanation:
All you have to do here is use the ideal gas law equation, which looks like this
∣
∣
∣
∣
¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯
a
a
P
V
=
n
R
T
a
a
∣
∣
−−−−−−−−−−−−−−−

, where
P
- the pressure of the gas
V
- the volume it occupies
n
- the number of moles of gas
R
- the universal gas constant, usually given as
0.0821
atm
⋅
L
mol
⋅
K

T
- the absolute temperature of the gas
Before plugging in your values, make sure that the units you have for volume and temperature match those used in the expression of the universal gas constant.
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Need
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Have
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Liters, L
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Liters, L
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√

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Kelvin, K
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Kelvin, K
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√
Since you already know the number of moles of gas present in your sample, you can proceed to solve the ideal gas law equation for
P
without making any unit conversions.
∣
∣
∣
∣
∣
¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯
a
a
P
V
=
n
R
T
⇒
P
=
n
R
T
V
a
a
∣
∣
∣
−−−−−−−−−−−−−−−−−−−−−−−−−−−
Plug in your values to get
P
=
0.540
moles
⋅
0.0821
atm
⋅
L
mol
⋅
K
⋅
223
K
35.5
L
P
=
∣
∣
∣
∣
¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯
a
a
0.278 atm
a
a
∣
∣
−−−−−−−−−−−−−
→
rounded to three sig figs

Mass is the amount of matter in an object.  weight is the measurement of the pull of gravity on an object.  say for example, you travel to the moon which has a different gravitational field compared to the gravitational field of earth. (gravitational fields: earth = 1, moon = 0.165)  now when you are on the moon, the pull of gravity on you is different than on the earth. and as weight is the measurement of the pull of gravity on an object, that means yes, your weight can and will change on the moon.  however, on the moon, on earth or even on jupiter, the amount of mass inside of you remains the same. meaning your physical mass remains constant.  in conclusion it is possible for your weight to change as your mass remains constant. 

Answerhave membrane-bound organelles;