a sample of gas has a volume 8 liters
@ 293 degree kelvin & 700 torr what will volume be at STP?
P1V1/T1=P2V2/T2 ; basic proportion.
STP mean standard temperature and pressure
P1=700 torr V1=8 Liters T1=293K
P2=standard pressure=1 atm=760 torr V2=unknown T2=standard temperature=273K
i hope you can follow my though process.
(700*8)/293=(760*V)/273
V=6.87
To find the volume of a gas 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
T = Temperature
At STP, the pressure is 1 atmosphere (atm) and the temperature is 273 Kelvin (K).
Given:
Volume (V1) = 8 liters
Temperature (T1) = 293 Kelvin (K)
Pressure (P1) = 700 torr
First, we need to convert the pressure from torr to atm.
1 atm = 760 torr
P1 = 700 torr / 760 torr/atm = 0.921 atm
Now we can solve for the number of moles (n) using the ideal gas law:
(P1)(V1) = (n)(R)(T1)
n = (P1)(V1) / (R)(T1)
Now we can substitute the given values:
n = (0.921 atm)(8 liters) / (0.0821 L·atm/mol·K)(293 K)
Calculating this expression, we can find the number of moles (n).
n ≈ 0.3017 moles
Now, we can find the volume at STP using the same relation with new pressure (P2) and temperature (T2):
P2 = 1 atm
T2 = 273 K
(P2)(V2) = (n)(R)(T2)
V2 = (n)(R)(T2) / P2
Substituting the values:
V2 = (0.3017 moles)(0.0821 L·atm/mol·K)(273 K) / (1 atm)
Calculating this expression, we can find the volume at STP (V2).
V2 ≈ 6.964 liters
Therefore, the volume of the gas at STP would be approximately 6.964 liters.
To find the volume of a gas at Standard Temperature and Pressure (STP), we need to use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
Before we can calculate the volume at STP, we need to convert the given temperature and pressure to Kelvin and atmospheres respectively.
Given:
Volume (V1) = 8 liters
Temperature (T1) = 293 Kelvin
Pressure (P1) = 700 torr
1. Convert the temperature to Kelvin:
To convert Kelvin to Celsius, we simply add 273 to the given temperature. So, T1 = 293K.
2. Convert the pressure to atmospheres:
Since 1 atmosphere is equal to 760 torr, we can calculate the pressure (P1) in atmospheres by dividing the given pressure by 760:
P1 = 700 torr / 760 torr/atm = 0.921 atm.
Now, we can calculate the volume (V2) at STP (Standard Temperature and Pressure). At STP, the temperature is 273 Kelvin and the pressure is 1 atmosphere.
3. Set up the ratio using the ideal gas law:
(V1 / T1) = (V2 / T2) * (P1 / P2)
Where T2 = 273K and P2 = 1 atm.
4. Rearrange the equation to solve for V2:
V2 = (V1 * T2 * P1) / (T1 * P2)
5. Substitute the values into the equation and calculate:
V2 = (8L * 273K * 0.921 atm) / (293K * 1 atm)
V2 = 6.29L
Therefore, the volume of the gas at STP would be approximately 6.29 liters.