Answer:
3.2 atm
Explanation:
To find the pressure inside the container when the volume is 70 cm^3, you can use the ideal gas law, which relates pressure (P), volume (V), and the number of moles (n) of a gas:
PV = nRT
Where:
P = Pressure (in atmospheres, atm)
V = Volume (in liters, L)
n = Number of moles
R = Ideal gas constant (approximately 0.0821 L·atm/(mol·K))
T = Temperature (in Kelvin, K)
In this case, you have the initial pressure (P1) and volume (V1) when the volume is 280 cm^3:
P1 = 0.8 atm
V1 = 280 cm^3 = 0.28 L (since 1 L = 1000 cm^3)
Now, you want to find the pressure (P2) when the volume is 70 cm^3:
V2 = 70 cm^3 = 0.07 L
You can set up a proportion using the ideal gas law for both initial and final conditions:
P1 * V1 = P2 * V2
Substitute the known values:
0.8 atm * 0.28 L = P2 * 0.07 L
Now, solve for P2:
P2 = (0.8 atm * 0.28 L) / 0.07 L
P2 = 3.2 atm
So, when the volume inside the container is 70 cm^3, the pressure is approximately 3.2 atm.