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At constant pressure how does the volume of 1 mole of an ideal gas vary?
Wiki User
∙ 8y ago
The volume varies inversely with pressure.
Wiki User
∙ 8y ago
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What is the volume of 3.5mol of CO2 gas at STP?
First convert the number of grams of CO2 into moles, then use the Ideal Gas Law. For how to solve this problem, see the two Related Questions links to the left of this answer.
How do I convert 76.0 grams of C4H10 to liters?
First, find out what the temperature and pressure of the gas is. Next, determine the mass per mole - this one I'll give you, it's 58.12 grams per mole. Divide 76 by 58.12 to get the number of moles of gas you have. Then, use the ideal gas law to determine the number of liters of gas per mole at the temp and pressure your gas is. Finally, multiply the liters per mole by the number of moles you have, and you've got it.
Calculate the mass of nitrogen dissolved at room temperature in an 96.0 home aquarium Assume a total pressure of 1.0 and a mole fraction for nitrogen of 0.78?
Using Henry's Law /// Solubility=(constant) (Pressure) We know that the mole fraction is equal to the partial pressure, so (.78atm) The constant at room temp, (from table) 6.1*10^-4 (M/atm) solubility = (6.1*10^-4)(.78) =4.758*10^-4 M So you just take your solubility (moles/L) x 92L to give you the number of moles =0.438moles times the g/mole of Nitrogen (N2) which is 28g/mol =1.2g I don't really understand how the other person did theirs, but I did not want to delete it, so it goes as follows: ______________________________________ .78/92=.84782 .84782 x 14.01= .11878 Move the decimal one over to the right. Answer= 1.2
At STP 0.250L of an unknown gas has a mass of 1.00 gram. Calculate its molar mass.?
1 standard volume of 1 mole of any gas @ STP is 22.4 LSo the # of moles in a 1 L sample will be:1 L*(1 mol/22.4 L) = 0.04464 molSince you already know the mass of the gas @ STP, the molar mass will be mass/#moles1.92 g/ 0.04464 mol = 43.01 g/mol
How is the volume of gas measured?
The volume of a gas is totally dependent on the container it is in, gas fills its container completely by its particles spreading out. The volume of the container is the same as volume of the gas inside the container. gasses are most commonly measured in SI units (Liters, mililiters, .....).
Explain why the molar volume of a gas at RTP is greater than that of the gas at STP?
At RTP the assumed temperature is 293ºK, at STP the assumed temperature is 273ºK. The formula used for this is Pressure x Volume = moles x ideal gas constant x Temperature. So Volume = (moles x ideal gas constant x temperature) / Pressure Assuming Pressure and moles stays constant... Volume at RTP = ( 1 mole x 8.31451 x 293 K ) / ( 101.325 Pa) Volume at RTP = 24.0429 Volume at RTP = 24.0dm^3 Volume at STP = ( 1 mole * 8.31451 * 273 K ) / ( 101.325 Pa) Volume at STP = 22.4017 Volume at STP = 22.4dm^3
What is the volume of a mole of any gas at standard temperature and pressure?
A mole of ideal gas at STP takes up 22.4 L.
If the temperature of a gas is constant and you multiply its pressure by its volume it will always equal the what?
Ideal gas Law PV = nRT where P is pressure V is volume n is moles R is a constant of 8.31 and T is temperature so if u multiply PV with T constant, that leaves nR, therefore you will always get mole of the air multiplied with 8.31
Is mole percent of a gas is equal to its volume percent?
Yes - as long as the pressure and temperature are constant.
What are the four variables in the ideal gas law?
Pressure, volume, temperature & the amount of gas.
At a constant temperature the pressure exerted by one mole of a gas decreases if the volume available is increased?
That is correct
When a mole of gas occupies 22.4 Liters this is known as?
This is the molar volume of an ideal gas at a given temperature and pressure.
What is constant for 1 mole of any ideal gas?
The Universal Gas Constant is 8.314 J/K/Mole
What is volume occupied by a mole of an ideal gas if the pressure is 626mmHg and the temperature is 25.0C?
I suppose that the correct anwer is 29,7 L.
State relation between mole fraction and Volume fraction?
For Ideal gases, mole fraction=volume fraction
What is the constant for 1 mole of any ideal gas?
The Universal Gas Constant is 8.314 J/K/Mole
When can volume fraction be equal to mole fraction?
The volume fraction of a substance is equal to the mole fraction for ideal gas mixture
