A cylinder at 48atm pressure and 290K releases 35ml of carbon dioxide gas into a 4.0L container at 297K. What is the pressure inside the container?

To solve this problem, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

First, let's calculate the number of moles of carbon dioxide gas released from the cylinder. We can use the ideal gas law equation to solve for n:

n = PV / RT

Given:
P = 48 atm
V = 35 ml = 0.035 L
R = 0.0821 L·atm/(mol·K)
T = 290 K

n = (48 atm * 0.035 L) / (0.0821 L·atm/(mol·K) * 290 K)
n ≈ 0.071 mol

Now, let's calculate the pressure inside the container. We can use the ideal gas law equation again:

P = nRT / V

Given:
n = 0.071 mol
R = 0.0821 L·atm/(mol·K)
T = 297 K
V = 4.0 L

P = (0.071 mol * 0.0821 L·atm/(mol·K) * 297 K) / 4.0 L
P ≈ 1.47 atm

Therefore, the pressure inside the container is approximately 1.47 atm.