Assuming the temperature and pressure are held constant, which of the gas samples has the greatest number of gas particles?
Answer
45.0 mL O3
35.0 mL N2
15.0 mL of CO2
25.0 mL of SO3
how would i go about answering this question.
1 mol of any gas occupies 22.4L and has 6.02E23 molecules(a molecule would count as one particle).
So 45.0 mL O3/22,400 = ? mol O3 and that x 6.02E23 = ? number molecules.
35.0/22,400 mL = ? mol O2 and x 6.02E23 = ?
15.0/22,400 = ? mol CO2 and x 6.02E23 = ?
25.0/22,400 = ? mol SO3 and x 6.02E23.
But if you will notice all of them are divided by 22,400 and all are multiplied by 6.02E23 so what does that tell you. First, that says you don't need to multiply and divide by all that stuff. That says that the largest number times two numbers that are constant will be the largest value of particles. right?
so it would be 45.0 mL O3
To determine which gas sample has the greatest number of gas particles, you can use the ideal gas law equation:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles
R is the ideal gas constant
T is the temperature
Under constant temperature and pressure conditions, the equation can be simplified to:
V/n = constant
This relationship implies that the volume of a gas is directly proportional to the number of moles. Therefore, the gas sample with the smallest volume will have the greatest number of gas particles.
To compare the gas samples and determine which has the smallest volume, you need to convert the given volumes to moles. To do this, you can use the ideal gas law equation and rearrange it to solve for n:
n = PV/RT
Plug in the given values for each gas sample, calculate the number of moles for each sample, and then compare the results. The gas sample with the smallest number of moles will indicate the greatest number of gas particles.