A 30.9 L cylinder containing C2H4F2 at a pressure of 114.0 torr is connected by a valve to 0.865 L cylinder containing C4H10 at 114.0 torr pressure. Calculate the partial pressure (atm) of C4H10 when the valve is opened.

i just need to know how to solve it i already know the answer

Use P1V1 = P2V2 for C4H10 and ignore the C2H4F2. You know P1, you're looking for P2, you know V1 = 0.865L and you know V2 (0.865L + 30.9L)

thankk you sooo much but what is

what is P2???

ohhhh waitt nevermind i got it:)

To calculate the partial pressure of C4H10 when the valve is opened, we need to use the ideal gas law.

The ideal gas law is given by the equation:
PV = nRT

Where:
P is the pressure of the gas
V is the volume of the gas
n is the number of moles of the gas
R is the ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature of the gas in Kelvin

First, let's calculate the number of moles of C2H4F2 in the 30.9 L cylinder.
Using the ideal gas law, we have:
n1 = (P1 * V1) / (R * T)

Since the problem states that the pressure is given in torr, we need to convert it to atm by dividing by 760.
P1 = 114.0 torr / 760 atm/torr = 0.15 atm

Now we can substitute the values:
n1 = (0.15 atm * 30.9 L) / (0.0821 L·atm/(mol·K) * T)

Next, we calculate the number of moles of C4H10 in the 0.865 L cylinder.
Using the ideal gas law, we have:
n2 = (P2 * V2) / (R * T)

Again, converting the pressure from torr to atm:
P2 = 114.0 torr / 760 atm/torr = 0.15 atm

Substituting the values:
n2 = (0.15 atm * 0.865 L) / (0.0821 L·atm/(mol·K) * T)

Since the cylinders are connected, when the valve is opened, the total number of moles of gas remains constant.
Therefore, n1 = n2.

Now we can equate the two expressions:
(0.15 atm * 30.9 L) / (0.0821 L·atm/(mol·K) * T) = (0.15 atm * 0.865 L) / (0.0821 L·atm/(mol·K) * T)

Rearranging the equation, we get:
30.9 / T = 0.865 / T
Dividing both sides by T, we get:
30.9 = 0.865

Simplifying further, we find:
T = 0.865 / 30.9
T = 0.0279 mol

Now we can calculate P2, the partial pressure of C4H10, by substituting the values into the ideal gas law equation:
P2 = (n2 * R * T) / V2

P2 = (0.0279 mol * 0.0821 L·atm/(mol·K) * 0.15 atm) / 0.865 L

Simplifying the expression, we find:
P2 = 0.00382 atm

Therefore, the partial pressure of C4H10 when the valve is opened is 0.00382 atm.