A0.5922 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as agcl by the addition of an excess of silver nitrate. the mass of the resulting agcl is found to be 1.3487 g. what is the mass percentage of chlorine in the original compound?

The mass percent chlorine in pure chloride compound is 56.31 %.

Explanation:

We are given:

Mass of AgCl precipitated = 1.3487 g

We know that:

Molar mass of AgCl = 143.32 g/mol

Molar mass of Chlorine atom = 35.45 g/mol

As, all the chlorine in the sample is precipitated to silver chloride. So, the mass of chlorine in silver chloride will be equal to the mass of chlorine present in the sample.

To calculate the mass of chlorine in given mass of AgCl, we apply unitary method:

In 143.32 g of silver chloride, mass of chlorine present is 35.45 g

So, in 1.3487 g of silver chloride, mass of chlorine present will be =

To calculate the percentage composition of chlorine in pure chloride compound, we use the equation:

Mass of pure chloride compound = 0.5922 g

Mass of chlorine = 0.3335 g

Putting values in above equation, we get:

Hence, the mass percent chlorine in pure chloride compound is 56.31 %.

b) mutualism

hope this : )

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.