PV=nRT
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Re: PV=nRT
P stands for pressure, V for volume, n for the moles of gas, R is a constant, T is the temperature.
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Re: PV=nRT
P is pressure, V is volume, n is # of moles of gas, R is the gas constant, T is temperature
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Re: PV=nRT
P is pressure, V is volume, n is the number of moles, R is the gas constant (it'll be given to us on the equations and constants sheet), and T is temperature.
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Re: PV=nRT
P is pressure in atm, V is volume in liters, n is the number of moles, R is the gas constant 8.206 x 10-2 L·atm·K-1·mol-1, and T is the temperature in Kelvin.
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Re: PV=nRT
P is pressure, V is volume, n is the number of moles, R is Rydberg's gas constant, and T is temperature.
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Re: PV=nRT
P = Pressure
V = Volume
n = number of moles
R = gas constant (in Kelvin)
T = Temperature (in Kelvin)
make sure all in right units
V = Volume
n = number of moles
R = gas constant (in Kelvin)
T = Temperature (in Kelvin)
make sure all in right units
Re: PV=nRT
You'll probably be using this formula whenever the question asks for one of the variables (pressure, volume, number of moles, or temperature) in relation to a gas and gives information that will help you derive the other variables in order to solve it
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Re: PV=nRT
P = pressure
V = volume
n = moles
R = gas constant (around 0.08206 I believe)
T = temperature in Kelvin
V = volume
n = moles
R = gas constant (around 0.08206 I believe)
T = temperature in Kelvin
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Re: PV=nRT
P = pressure
V = volume (usually in liters)
n = moles
R = gas constant
T = temperature (usually in kelvin)
Make sure to be extra careful with units as there are different gas constants based on the different units used for the pressure. For example, there is a different gas constant depending on if the desired or given pressure is atm, bars, etc. Additionally, make sure to convert volumetric units to liters as our gas constants always use liters. Temperature in the gas constant is always in kelvin, while questions may be given in either celsius or kelvin (probably not fahrenheit). To get kelvin from celsius, just add 273.
V = volume (usually in liters)
n = moles
R = gas constant
T = temperature (usually in kelvin)
Make sure to be extra careful with units as there are different gas constants based on the different units used for the pressure. For example, there is a different gas constant depending on if the desired or given pressure is atm, bars, etc. Additionally, make sure to convert volumetric units to liters as our gas constants always use liters. Temperature in the gas constant is always in kelvin, while questions may be given in either celsius or kelvin (probably not fahrenheit). To get kelvin from celsius, just add 273.
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Re: PV=nRT
P is pressure, and the SI unit is Pascals but often we use bar or atm (be careful to look out for this because it will change which gas constant R you use)
V is volume in liters or m^3
n is the moles
R is the gas constant (varies with pressure and volume)
T is the temperature (in Kelvin)
conversion is K = C˚ + 273.15
V is volume in liters or m^3
n is the moles
R is the gas constant (varies with pressure and volume)
T is the temperature (in Kelvin)
conversion is K = C˚ + 273.15
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Re: PV=nRT
P= pressure (units: atm)
V = volume ((units: Liters)
n = (units: mols)
R = constant (units: L atm mol-1K-1)
T = temperature ((units: Kelvin)
* The units are very important for the equation. Make sure that temperature is in Kelvin, volume is in Liters, and pressure in atm. Those are usually the ones that can be given in different units in problems.
V = volume ((units: Liters)
n = (units: mols)
R = constant (units: L atm mol-1K-1)
T = temperature ((units: Kelvin)
* The units are very important for the equation. Make sure that temperature is in Kelvin, volume is in Liters, and pressure in atm. Those are usually the ones that can be given in different units in problems.
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Re: PV=nRT
FionaHunter21 wrote:So is R the same constant as the one we used before on the equation sheet?
No the R constant on the equation sheet we have is in hertz which is not useful to us when using this equation so the R constant in this case could be 0.08205746 L⋅atm/mol⋅K but could be different depending what units you use.
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Re: PV=nRT
Leslie Almaraz 4G wrote:when do you know you are allowed to use this formula?
You would be using this formula if you want to convert between partial pressures and concentrations. For example, if the problem asks you to solve for Kc but you are only given partial pressures, you can plug these values into the equation to get their concentrations (n/V) and solve for Kc. Hope this helps!
Re: PV=nRT
Leslie Almaraz 4G wrote:when do you know you are allowed to use this formula?
Hey Leslie,
Just like Alexandra said, you can use this idea gas formula to convert from the concentration Kc to the partial pressure Kp, and vise versa. In order to do that, you would divide V (the volume) by both sides to isolate the P (or Kp); which looks like P=(n/v)RT. From there, n/v basically would be the concentration Kc, which is were you would plug in the Kc in order to find Kp.
I hope this helps!!!
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Re: PV=nRT
P = pressure in atm
V = volume in L
n = amount of substance in moles
R = gas constant (0.08206 J*K[*]-1 M[*]-1)
T = temperature in Kelvin
V = volume in L
n = amount of substance in moles
R = gas constant (0.08206 J*K[*]-1 M[*]-1)
T = temperature in Kelvin
Re: PV=nRT
FionaHunter21 wrote:So is R the same constant as the one we used before on the equation sheet?
Hey Fiona, the R constant would be gas constant which is 0.082057 L atm mol^-1 K^-1.
Hope this helps!
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Re: PV=nRT
P=pressure (in atm)
V=volume of gas (in L)
n= number of moles
R= gas constant
T= temperature (in Kelvin)
n/V = concentration
V=volume of gas (in L)
n= number of moles
R= gas constant
T= temperature (in Kelvin)
n/V = concentration
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Re: PV=nRT
P = Pressure (in atm)
V = Volume (in L)
n = # of moles
R = gas constant
T = Temperature (in K)
remember to use SI units!
V = Volume (in L)
n = # of moles
R = gas constant
T = Temperature (in K)
remember to use SI units!
Re: PV=nRT
P= pressure (atm); V= volume (Liters); n=moles; R=gas constant (no units needed); T=temperature (Kelvin)
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Re: PV=nRT
P is pressure, V is volume, n is number of gaseous moles, R is the gas constant, T is temperature in Kelvin.
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Re: PV=nRT
P is Pressure, V is Volume, n is number of moles, R is the gas constant, and T is Temperature
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Re: PV=nRT
P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is the temperature.
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Re: PV=nRT
P = pressure, V = volume, n = number of moles, R = constant, T = temperature in Kelvin (I always forgot that T should be in K haha)
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Re: PV=nRT
P is for pressure, V is for volume, n is number of moles of gas, R is the gas constant, T is for temperature
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Re: PV=nRT
P is pressure, V is volume in liters, n is moles, R is a constant (that changes depending on the unit of pressure), and T is temperature (in Kelvin)
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Re: PV=nRT
P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is temperature. You can manipulate this equation in several ways, one of which being P= (n/V)*RT which can also be rewritten as P=concentration*RT because (n/V) is how concentration is calculated.
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Re: PV=nRT
P= pressure, V= volume, n= number of moles, R= gas constant, and T= temperature (in Kelvin).
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Re: PV=nRT
P = pressure (atm)
V= Volume (L)
n = number of mols
R = gas constant (which is given)
T = temp (Kelvin)
V= Volume (L)
n = number of mols
R = gas constant (which is given)
T = temp (Kelvin)
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Re: PV=nRT
P= pressure in atm
V= volume in liters
n= number of moles
R= gas constant (8.31446261815324 J⋅K−1⋅mol−1)
T= temperature in Kelvin
V= volume in liters
n= number of moles
R= gas constant (8.31446261815324 J⋅K−1⋅mol−1)
T= temperature in Kelvin
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Re: PV=nRT
P=Pressure in atm
V=Volume in Liters
n=number of moles
R=Gas Constant
T=Temperature (always in Kelvin cause of R's units I believe—to convert from Celsius add 273.15)
V=Volume in Liters
n=number of moles
R=Gas Constant
T=Temperature (always in Kelvin cause of R's units I believe—to convert from Celsius add 273.15)
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Re: PV=nRT
For PV=nRT,
P stands for pressure
V for volume
n for amount of moles
R for the gas constant, equaling 8.314 J/mol·K
T for temperature
P stands for pressure
V for volume
n for amount of moles
R for the gas constant, equaling 8.314 J/mol·K
T for temperature
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Re: PV=nRT
P is for Pressure, V is for Volume in Liters, n is for number of moles, R is for gas constant, and T is for Temperature in Kelvin
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Re: PV=nRT
P = Pressure, usually given in Bars / atm
V = Volume, in Liters
n = number of mols
R = The gas constant, equal to 8.3145 J mol^-1 K^-1
T = Temperature in Kelvin
V = Volume, in Liters
n = number of mols
R = The gas constant, equal to 8.3145 J mol^-1 K^-1
T = Temperature in Kelvin
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Re: PV=nRT
P = Pressure, typically in atm or bars
V = Volume, Liters
n = # of moles
R = gas constant (which I believe is provided on the equations sheet)
T = temperature, Kelvin
V = Volume, Liters
n = # of moles
R = gas constant (which I believe is provided on the equations sheet)
T = temperature, Kelvin
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Re: PV=nRT
P: pressure (units: atm)
V: volume (units: Liters)
n: moles (unit: mol)
R: constant (should match the other units in the equation) --> value = 8.314
T: temperature (units: Kelvin)
*It is very important to make sure you plug in the correct units into each variable in the equation. Pressure, volume, and temperature are the most missed variables because there is a higher chance that the value given in the problem will have different units.
V: volume (units: Liters)
n: moles (unit: mol)
R: constant (should match the other units in the equation) --> value = 8.314
T: temperature (units: Kelvin)
*It is very important to make sure you plug in the correct units into each variable in the equation. Pressure, volume, and temperature are the most missed variables because there is a higher chance that the value given in the problem will have different units.
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Re: PV=nRT
Does anybody know when exactly we need to use this equation? I haven't encountered it in any of the textbook problems.
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Re: PV=nRT
P stands for Pressure, V stands for Volume, n stands for number of moles, R stands for gas constant, T stands for temperature.
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