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What else can I help you with?
The volume of a gas is directly proportional to the number of moles of that gas if?
the pressure and temperature are held constant. ideal gas law: Pressure * Volume = moles of gas * temperature * gas constant
Volume temperature pressure?
P1V1=P2V2 P1V1/T1=P2V2/T2 PV=nRT P=pressure V=volume n=number of moles R=the gas constant 8.31J/molK or 0.0821Latm/molK T=temperature in kelvin
What type of relationship do volume and temperature have?
According to Charles law,the given volume is directly proportional to the absolute temperature at constant pressure and number of moles. "Asad Jamal" HAMDARD UNIVERSITY Karachi,Pakistan.
Moles of gases at standard temperature pressure?
... "are proportional to the volume they occupy, divided by their specific gas constant." With P and T constant... V1 / (n1 R1) = V2 / (n2 R2) = ...
What are three measurements that are helpful when working with a gas?
Temperature, Pressure, # of moles, volume of container. If you know any three of those you can find the remaning by equation PV=nRT, where P=pressure in atmospheric units, V=volume in liters, n=number of moles of the gas, R=universal gas constant (which, in this formula, is equivalent to .08206), and T=temperature in Kelvins (not centigrade, but kelvins).
What pressure in atmosphere will 10.7 moles of He exert when it is compressed in a 16.0 liter tank at a temperature of 50 C?
The pressure is 17,8 atmospheres.
What is the pressure of 4 moles of helium in a 50 liter tank at 308k?
Using the ideal gas law (PV = nRT), where P is pressure, V is volume, n is number of moles, R is the ideal gas constant, and T is temperature in Kelvin, we can solve for pressure. Plugging in the values, the pressure of the 4 moles of helium in a 50 liter tank at 308 K is approximately 81.6 atm.
How do you solve What is the pressure in a canister of argon gas 56.72 g at 23 degrees C?
To find the pressure in the canister, you will need to use the ideal gas law equation, PV = nRT. First, convert the mass of argon into moles using the molar mass of argon (39.95 g/mol). Then, rearrange the equation to solve for pressure (P) and plug in the known values: n (moles), R (gas constant), T (temperature in Kelvin), and V (volume, if available).
How many moles of O2 gas in 1L container?
I assume you mean at standard temperature and pressure. Use, PV = nRT (1 atm)(1 liter) = n(0.08206 L*atm/mol*K)(298.15 K) n = 1/24.466 = 0.04 moles oxygen gas --------------------------------
When is pressure useful?
when determining volume, moles, weight, and/or temperature
The volume of a gas is directly proportional to the number of moles of that gas if?
the pressure and temperature are held constant. ideal gas law: Pressure * Volume = moles of gas * temperature * gas constant
What is the pressure of 4 moles of helium in a 50 liter tank at 308 kelvins using PVnRT?
The pressure will be 2,02 atmospheres.
What is the relationship between temperature, volume, pressure, and the number of moles of a gas as described by the ideal gas law equation w-nRT?
The ideal gas law equation, w-nRT, describes the relationship between temperature (T), volume (V), pressure (P), and the number of moles of a gas (n). It states that the product of pressure and volume is directly proportional to the product of the number of moles, the gas constant (R), and the temperature. In simpler terms, as temperature increases, the volume of a gas increases if pressure and the number of moles are constant. Similarly, if pressure increases, volume decreases if temperature and the number of moles are constant.
How many moles is 15.2L of CH4?
It depends on temperature,pressure and volume.THese are needed to find number of moles
How many moles of gas occupy 1.3 L at a pressure of 3.89 atmospheres and a temperature of 323 K?
The answer is 0,19 moles.
If the volume and number of moles of gas are held constant as the temperature increase what will the pressure do?
If the volume and number of moles of gas are constant, then according to the ideal gas law, pressure is directly proportional to temperature. As temperature increases, the pressure will also increase in order to maintain equilibrium.
What is the standard temperature and pressure for 6.00 moles of Br2?
For chemistry, after IUPAC rules the standard temperature is 0 oC and the standard pressure is1 bar.
