8.........................................................................................
Answer:
describes properties characteristic of no more than two electrons in the vicinity of an atomic nucleus or of a system of nuclei as in a molecule
The empirical formula of the compound is calculated as follows:
Given that
It contains 85.63% carbon, and 100-85.63= 14.37 % hydrogen
now assume that the amount of compound is100 g thus there is 85.63 g C and 14.37 g H
NOW divide these percentages by the molar mass of the elements to get a number of moles for each substance.
NUMBER OF MOLES = AMOUNT IN G / MOLAR MASS
Carbon: 85.63/12 = 7.1
Hydrogen: 14.37/1 = 14.3
Now arrange these in a ratio as follows:
C:H
7.1/7.1 :14.3/7.1
1:2
divide through by the smallest number
Therefore, the empirical formula is CH2
Then calculate the molar mass of that molecule:
(1x12) + (2x1) = 14
Here the molar mass of compound is 56.10 g/mol
Since, 14 goes into 56.10 g/mol 4 times thus the molecular formula is : C4H8
Answer:
The pressure contribution from the heavy particles is 17.5 atm
Explanation:
According to Dalton's law of partial pressures, if there is a mixture of gases which do not react chemically together, then the total pressure exerted by the mixture is the sum of the partial pressures of the individual gases that make up the mixture.
In the simulation:
the pressure of the 50 light particles alone was determined to be 5.9 atm, the pressure of the 150 heavy particles alone was measured to be 17.5 atm,
the total pressure of the mixture of 150 heavy and 50 light particles was measured to be 23.4 atm
Total pressure = partial pressure of Heavy particles + partial pressure of light particles
23.4 atm = partial pressure of Heavy particles + 5.9 atm
Partial pressure of Heavy particles = (23.4 - 5.9) atm
Partial pressure of Heavy particles = 17.5 atm
Therefore, the pressure contribution from the heavy particles is 17.5 atm