At 1.70 atm, a gas sample occupies 4.25 liters. If the pressure in the gas increases to 2.40 atm, what will the new volume be?
Answer:
3.01L
Explanation:
Given parameters:
Initial pressure, P1 = 1.7atm
Initial volume, V1 = 4.25L
Final pressure, P2 = 2.4atm
Unknown:
Final or new volume, V2 = ?
Solution:
To solve this problem, we use Boyle's law which states that "the volume of a fixed mass of a gas varies inversely as the pressure changes, if the temperature is constant".
P1 V1 = P2 V2
P1 is the initial pressure
V1 is the initial volume
P2 final pressure
V2 final volume
1.7 x 4.25 = 2.4 x V2
V2 = 3.01L
<span>The momentum of the second ball will depend on the acceleration of the first moving ball.</span>
Answer:
4.88 K.
Explanation:
From the question given above, the following data were obtained:
Number of mole (n) = 5 moles
Pressure (P) = 1 atm
Volume (V) = 2 L
Gas constant (R) = 0.082 atm.L/Kmol
Temperature (T) =?
The temperature of the gas can be obtained by using the ideal gas equation as illustrated below:
PV = nRT
1 × 2 = 5 × 0.082 × T
2 = 0.41 × T
Divide both side by 0.41
T = 2 / 0.41
T = 4.88 K
Therefore, the temperature of the gas is 4.88 K.
Answer:
D, using a spring scale to exert a force on the block. Measure the acceleration of the block and the applied force
Explanation:
For this you would use the net force equation acceleration=net force * mass however you will want to isolate mass so it would be acceleration/ net force to get mass. Then process of elimination comes to play.
Answer:
91.21
Explanation:
Kinetic energy =1/2 mv2 substitute the values I. E 1/2 *1 *4.5^2= 91.21
