The air in a 5.00L tank has a pressure of 1.20atm. What is the new pressure of the air when the air is placed in tanks that have the following volumes, if there is no change in temperature?
A. 1.00L B. 2500ml C. 750ml
To solve this problem, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional when temperature is constant.
Boyle's Law can be expressed as:
P1 * V1 = P2 * V2
Where:
P1 and V1 are the initial pressure and volume
P2 and V2 are the final pressure and volume
Given:
Initial volume (V1) = 5.00L
Initial pressure (P1) = 1.20atm
Let's calculate the new pressures for each given volume:
A. 1.00L:
P1 * V1 = P2 * V2
1.20atm * 5.00L = P2 * 1.00L
P2 = (1.20atm * 5.00L) / 1.00L
P2 = 6.00atm
B. 2500ml:
First, convert 2500ml to liters by dividing by 1000:
2500ml / 1000 = 2.50L
P1 * V1 = P2 * V2
1.20atm * 5.00L = P2 * 2.50L
P2 = (1.20atm * 5.00L) / 2.50L
P2 = 2.40atm
C. 750ml:
First, convert 750ml to liters by dividing by 1000:
750ml / 1000 = 0.75L
P1 * V1 = P2 * V2
1.20atm * 5.00L = P2 * 0.75L
P2 = (1.20atm * 5.00L) / 0.75L
P2 = 8.00atm
Therefore, the new pressures of the air when placed in tanks with the given volumes are:
A. 6.00atm
B. 2.40atm
C. 8.00atm