The gas molecules move between the system and the surroundings follow PV=nRT.
<h3>What are molecules?</h3>
The smallest particle of a substance has all of the physical and chemical properties of that substance.
An increase in pressure pushes the molecules closer together, reducing the volume. If the pressure is decreased, the gases are free to move about in a larger volume.
In the kinetic theory of gasses, increasing the temperature of a gas increases in average kinetic energy of the molecules, causing increased motion.
The reduction in the volume of the gas means that the molecules are striking the walls more often increasing the pressure, and conversely if the volume increases the distance the molecules must travel to strike the walls increases and they hit the walls less often thus decreasing the pressure.
At constant temperature and pressure the volume of a gas is directly proportional to the number of moles of gas. At constant temperature and volume the pressure of a gas is directly proportional to the number of moles of gas.
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Answer:
Explanation:
91.4
grams
Explanation:
C
=
m
o
l
v
o
l
u
m
e
2.45
M
=
m
o
l
0.5
L
2.45
M
⋅
0.5
L
=
m
o
l
m
o
l
=
1.225
Convert no. of moles to grams using the atomic mass of K + Cl
1.225
m
o
l
⋅
(
39.1
+
35.5
)
g
m
o
l
1.225
m
o
l
⋅
74.6
g
m
o
l
=
1.225
⋅
74.6
g
=
91.4
g
Answer:
6.4g
Explanation:
32g of O2 produce 36g of H2O/5.70g of O2 produce x the answer is 6.4g
