Answer:
Kinetic theory explains why the volume of a container must expand when the temperature of the gas inside increases in order for the pressure to remain constant.
Step-by-step explanation:
Charles' law: for a fixed mass of gas at constant pressure the volume is directly proportional to the temperature.
Analysis of a gas when its temperature increases according to kinetic theory:
The temperature has increased therefore the molecules have more kinetic energy, so they move with a greater velocity.¹
If the container's dimensions do not change the molecules will travel across the container between the walls in less time (because they are moving faster and covering the same distance between the container walls). This will increase the rate of collisions, which would increase the pressure.²
But if the dimensions of the container increased then the molecules would cover a larger distance faster thereby maintaining a constant rate of collisions. This would maintain a constant pressure.
GP = 1/2 , 1/4 , 1/8 , 1/16
1st) the common ratio is (1/4 : 1/2 ) = 1/2, so r =1/2
2nd) the sum of a GP is:
S= a(1-rⁿ)/(1-r)
S=(1/2).[1-(1/2)⁴]/(1-1/2) = 15/16
Flat rate=y intercept
rate per mile=slope
y=3x+10 would be it
1.
3 is the value of the slope (3 dollars per mile)
2.
y intercept is (0,10)
3.
22 miles
y=3(22)+10
y=66+10
y=76
$76
((7 + 5)^2) / (4 * 3 + 9) =
(12^2) / (12 + 9) =
144 / 21 reduces to 48/7 or 6 6/7
Answer:
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Step-by-step explanation:
