You really should do your own homework.
PV = nRT ==> V = nRT/P
T = 15 c = 288.15 K
P = 1.10 ATM (gauge) = 2.1 ATM (absolute) = 212.783 kPa
R = 8314.472 kPa cm^3/(gram mole deg K)
n = 600 gram moles
V = 600 gram moles x 8314.472 kPa cm^3/(mole K) x 288.15 K / 212.783 kPa 6.756 x 10^6 cm^3 6,759 liters
288 K or 15 C
What is the volume of a 24.7 mol gas sample that has a pressure of .999 ATM at 305 K?
cos2(s)
increases......
A sample of gas occupies 1.55L at STP. What will the volume be if the pressure is increased to 50 atm while the temperature remains constant?
288 K or 15 C
in order to calculate the mean of the sample's mean and also to calculate the standard deviation of the sample's
The pressure of a sample of helium in a 1.00- L container is 0.988 atm. What is the new pressure if the sample is placed in a 200- L container
More pressure means less volume. Calculate the ratio of pressure, then divide the 4.2 liters by that ratio.This assumes: * That the temperature doesn't change. * That the gas behaves like an ideal gas.
We would need to know what sample you are referring to in order to answer this question.
See related link.
Count up the number of obseravtions made on the experimental units. That is the sample size.
10.81x10^6amu
Density of a substance = (mass of a sample of the substance) divided by (volume of the same sample)
i dont no the answer
Standard error of the sample mean is calculated dividing the the sample estimate of population standard deviation ("sample standard deviation") by the square root of sample size.
You solve this by using the ideal gas law: PV=nRT, where P, V, and T are pressure, volume, and temperature (in kelvins), R is the "ideal gas constant" with a value of approx. 0.08, and n is the number of moles. Plugging it in, we get: 2.75(V) = 880(0.08)(254) *note that we converted Celsius to kelvins by adding 273. Solving for "V" we get 6,502.4 liters.