Answer:
Molar mass = 254.60g/mol
Step-by-step explanation:
Mass = 8.02g
Volume = 812mL = 0.812L
Pressure (P) = 0.967atm
Temperature of the gas = 30°C = (30 + 273.15)K = 303.15K
Molecular weight = ?
To solve this question, we'll have to use ideal gas equation, PV = nRT
P = pressure of the gas
V = volume of the gas
n = number of moles of the gas
R = ideal gas constant = 0.082J/mol.K
T = temperature of the gas
PV = nRT
n = PV / RT
n = (0.967 * 0.812) / (0.082 * 303.15)
n = 0.7852 / 24.8583
n = 0.0315 moles
Number of moles = mass / molarmass
Molarmass = mass / number of moles
Molar mass = 8.02 / 0.0315
Molar mass = 254.60g/mol
The molar mass of the gas is 254.60g/mol
Answer:

Step-by-step explanation:
the mean is given by:

In our case this is:

side note: the main difference between sample mean and population mean is in the 'context'. However, the method to calculate them is the same.
By context I mean: if this the items are taken from some larger category for example: the ages of a few 'students' from a 'class'. Here 'students' are the sample from a larger set that is 'class'. The mean of the 'few students' will be called sample mean. In contrast, if we take the mean of the ages of the whole class then this is called population mean. (population mean == mean of the whole set)
In our case we aren't told exactly where these numbers come from, is this the whole set or a sample from it, the lack of context allows us to assume that the mean can either be population mean or sample mean. So we can safely use any symbol
or
.
The 2nd place after(to the right) the decimal. For example: .01. 1 would be in the hundredth place.