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.