Achloride of silicon contains 79.1 mass % cl. (a) what is the empirical formula of the chloride?

SiCl₃

Explanation:

To solve this problem, let's assume that we have 100 g of that chloride of silicon. We then would have 79.1 g of Cl and 100 - 79.1=20.9 g of Si.

Then we calculate the amount of moles in the mass of each element, using the elements' atomic weight:

Now we divide the number of moles by the lowest number, in this case, it's the moles of Si:

2.2313 / 0.7443 = 2.9978 => 3

0.7443 / 0.7443 = 1

Thus the empirical formula is SiCl₃

i believe it is-

d.) gravity pulled particles of dust and gas together to form planets.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.