the volume of a sample of gas is 650.ml at STP. what volumes will the sample occupy at 0.0degrees celsius and 950.torr???
is it 650.ml?
The volume to start with is 650 and you've increased pressure. It can't stay the same.
P1V1 = P2V2
thanks..... andy
Well, if you're looking for a serious answer, no, the volume of the sample will not remain exactly 650 mL at 0.0 degrees Celsius and 950 torr. The volume of a gas is affected by changes in temperature and pressure, so it will likely be different. However, if you're looking for a funny response, let's just say that the gas has a knack for keeping the same volume no matter what the conditions are - it's a real volume-chameleon! You can't underestimate its commitment to staying at 650 mL, no matter how cold or how under pressure it may be!
To determine the volume of a gas sample at different conditions, 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)
At standard temperature and pressure (STP), the conditions are 0 degrees Celsius and 1 atmosphere (atm). To convert 0 degrees Celsius to Kelvin, we add 273.15:
T1 = 0 + 273.15 = 273.15 K
P1 = 1 atm
Using the ideal gas law, we can determine the number of moles of gas:
PV = nRT
(1 atm)(650 ml) = n(0.0821 L·atm/(mol·K))(273.15 K)
650 ml = n(0.0821)(273.15)
n = (650 ml)/(0.0821)(273.15)
Now, to determine the volume at new conditions of 0 degrees Celsius and 950 torr, we convert the pressure from torr to atm:
P2 = 950 torr / 760 torr/atm = 1.25 atm
Using the new pressure and the same number of moles (n), we can calculate the volume:
PV = nRT
(1.25 atm)(V2) = n(0.0821)(273.15)
V2 = (n(0.0821)(273.15))/(1.25)
Substituting the calculated value of n, we can find the volume at the new conditions:
V2 = ((650 ml)/(0.0821)(273.15))(0.0821)(273.15)/(1.25)
Simplifying the equation:
V2 = (650 ml)(0.0821)(273.15)/(1.25)
Using a calculator to solve the equation, we find:
V2 ≈ 431.94 ml
So, the volume of the gas sample at 0 degrees Celsius and 950 torr would be approximately 431.94 ml, not 650 ml.
To determine the volume of a sample of gas at a different temperature and pressure, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = moles of gas
R = ideal gas constant
T = temperature in Kelvin
At STP (standard temperature and pressure), the temperature is 273.15 K and the pressure is 1 atmosphere.
Given:
Initial volume (V1) = 650 mL
Initial temperature (T1) = 273.15 K at STP
Initial pressure (P1) = 1 atmosphere at STP
We can find the initial number of moles of gas (n1) using the ideal gas law:
n1 = (P1 * V1) / (R * T1)
Now, we want to determine the new volume (V2) at a different temperature (T2) and pressure (P2):
T2 = 0.0°C + 273.15 = 273.15 K
P2 = 950 Torr
R = 0.0821 L·atm/mol·K (ideal gas constant)
To find V2, we rearrange the ideal gas law equation and solve for V2:
V2 = (n1 * R * T2) / P2
Let's calculate V2 using the given values:
n1 = (1 atm * 650 mL) / (0.0821 L·atm/mol·K * 273.15 K)
n1 = 0.02618 moles (approximately)
V2 = (0.02618 moles * 0.0821 L·atm/mol·K * 273.15 K) / 950 Torr
V2 ≈ 0.618 L (or 618 mL)
Therefore, the sample of gas will occupy approximately 618 mL at 0.0 degrees Celsius and 950 Torr, not 650 mL.