If you are given
V1=410 ml
T1= 27 C= 300 K
P1= 740 mm
Find
V2 in ml at STP
When given STP= 273K and 1 atm
(P1V1/T1) = (P2V2/T2)
I have this formula and I plugged in the given information.
740mm(410ml)/300K but I don't know what my P2 would be?
P2 is 1 atm. Since you must use the same units for P1 and P2, since P1 is in mm Hg, I would convert 1 atmosphere to mm Hg. That is 760 mm Hg.
(740*410/300) = (760*V2/273)
Solve for V2.
okay thank you!
To find V2 at STP (Standard Temperature and Pressure), we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant (0.0821 L * atm / (mol * K))
T = Temperature in Kelvin
Given:
V1 = 410 ml
T1 = 27 °C = 300 K
P1 = 740 mmHg
First, we need to convert the pressure from mmHg to atm. Since 1 atm = 760 mmHg, we can calculate P1 in atm:
P1 = 740 mmHg / 760 mmHg/atm ≈ 0.974 atm
Next, assuming the number of moles (n) remains constant, we can rearrange the equation to solve for V2:
V2 = (n * R * T2) / P2
Since we are given STP conditions:
T2 = 273 K
P2 = 1 atm
Substituting the values into the equation:
V2 = (n * R * 273 K) / 1 atm
Now, to solve for V2, we need to find the number of moles (n). To calculate moles, we can use the ideal gas law equation:
PV = nRT
Rearranging the equation to solve for n:
n = (PV) / (RT)
Substituting the known values and solving for n:
n = (0.974 atm * 410 ml) / (0.0821 L * atm / (mol * K) * 300 K)
n ≈ 18.5 mol
Finally, substituting the values of n and the given values of R, T2, and P2 into the equation for V2:
V2 = (18.5 mol * 0.0821 L * atm / (mol * K) * 273 K) / 1 atm
After calculating the above expression, you will find the value of V2 in liters. To convert it to milliliters, you can multiply it by 1000:
V2 = (18.5 mol * 0.0821 L * atm / (mol * K) * 273 K) / 1 atm ≈ 435 ml
Therefore, V2 at STP is approximately 435 ml.