Use the ideal gas law, PV=nRT, in which P= pressure, V= volume, n= number of moles, R= the gas constant, and T= temperature. In this problem you know V, T, R, and n. What you are trying to figure out is the P.
P= Unknown
V= 35.0 L
n= 6.50 moles
R= .082057 L ATM/mol K
T= 305 K
PV= nRT
P35.0=6.50(.082057)305
P= 4.65 ATM
This is an ideal gas law problem, PV=nRT, where p = 14 atm, V = 35 L, n = 9 mol, R = 0.082 L atm/mol K.
Rearrange the equation to solve for T:
T=(PV)/(nR)
T=(14 atm x 35 L)/(9 mol x 0.082 L atm/mol K) = 700 K if your teacher is counting significant figures, 664 K if she isn't.
This problem can be solved with the ideal gas law. The original pressure and volume of the container are proportional the final pressure and volume of the container. The original pressure was 1 atmosphere and the original volume was 1 liter. If the final volume is 1.8 liters, then the final pressure is 0.55 atmospheres.
0.5atm
It would contain about that much gas. As much as u put into it.
The pressure is never low enough, nor the temperature high enough to get a perfect match; but at room temp it comes pretty close. This is the answer: 750 K and 20 kPa (I AM THE WISEONE!!)
Hydrogen? You need the conditions, pressure and temperature, of the gas. 1 mole of the gas occupies 22.4 liters at STP. The molar mass of hydrogen is 2.0 g/ mole. So the density at STP is 2.0 / 22.4 = 0.0893 g/liter. At any other pressure and temperature you can use the ideal gas law to find the volume of one mole and then find the density.
Use Boyle's Law, applicable for ideal gases at constant temperature, to solve this problem: P1*V1 = P2*V2
This problem can be solved with the ideal gas law. The original pressure and volume of the container are proportional the final pressure and volume of the container. The original pressure was 1 atmosphere and the original volume was 1 liter. If the final volume is 1.8 liters, then the final pressure is 0.55 atmospheres.
0
This looks suspiciously like a homework question! Temp of 8 mol of ideal gas in a 32 L container at 12 atm pressure? pV = 12 * 32 = 384 L.atm nRT = 8 * 0.082 * T = 0.656 * T L.atm T = 384/0.656 = ~516 K That should provide the template for your answer!
The volume doubles
0.5atm
To find the temperature, we can use the ideal gas law equation: PV = nRT. Rearranging the equation to solve for temperature (T), we have T = (PV) / (nR), where P is the pressure, V is the volume, n is the number of moles, and R is the ideal gas constant. Plugging in the given values (P = 20 kPa, V = 100 L, n = 1 mol, and R = 8.314 J/(molยทK)), we find that the temperature is approximately 239 K.
Gas pressure depends on volume, temperature, AND the amount of gas. You didn't give an amount of gas, so there is no way to answer your question.
1 liter of water weight about 1 kilo. (The exact weight depends on the pressure and temperature). Therefore the container above holds 3.2 liters.
It would contain about that much gas. As much as u put into it.
There is most likely a more efficient way to do this, but this is the best I can do for now.Notation: ( x , y ) where x is the amount of water in the 5-liter container and y is the amount of water in the 7-liter container1. Fill the five-liter container ( 5 , 0 )2. Pour the five-liter container into the seven-liter container ( 0 , 5 )3. Fill the five-liter container ( 5 , 5 )4. Fill the seven-liter container with the five-liter container, leaving 3 liters in the five-liter container ( 3 , 7 )5. Pour out the seven-liter container ( 3 , 0 )6. Pour the five-liter container into the seven-liter container ( 0 , 3 )7. Fill the five-liter container ( 5 , 3 )8. Fill the seven-liter container with the five-liter container, leaving 1 liter in the five-liter container ( 1 , 7 )9. Pour out the seven-liter container ( 1 , 0 )10. Pour the five-liter container into the seven-liter container ( 0 , 1 )11. Fill the five-liter container ( 5 , 1 )12. Pour the five-liter container into the seven-liter container ( 0 , 6 )
When the volume of an "ideal gas" increases AND the amount (number of moles*) of gas remains constant, the temperature of the gas will decrease. One relevant assumption for an "ideal gas" is that it is "dry" - no water vapor (humidity) in the sample One relevant equation is the Ideal Gas Law P*V = n*R*T When P = pressure in atmospheres V = volume in liters n = amount of the Ideal Gas, in moles R = the ideal, or universal, gas constant = 0.08206 L*atm / mol * K which is read as "liter-atmospheres per mole-Kelvin" T = the absolute temperature in K, "Kelvins" *A "mole" is 6.022×1023 atoms or molecules of a substance. This is known as "Avogadro's Number"