Chemistry work :(

Question

A compound has the empirical formula CHF. A 256-mL flask, at a 373 K and 750 torr, contains 0.527g of the gaseous compound. Give the molecular formula

Answer 1

Awful question, very scary. This is how I start: it's a gas, so I'm gonna pull out PV = nRT

0.527g of the compound will help us find n eventually,

V is 256 ml since a gas fills the container it's in,

T is 373 Km

P is 750 torr,

and R we will have to select to fit the units we were given, or change them to fit.

SO, we can see the only value not given is n, so solve for n. (I'm not going to do this for you, that might be cheating and I'm new here). However, the R value I recommend using is 62.363 because its units are Liters * Torr / K / mol

Once you get an n value, we know how many moles are in this flask. Now we have moles, the mass in grams, and the constituent elements (CHF). Find the atomic mass of this base empirical formula, which I'll denote as [CHF]

n moles of x[CHF] = grams, right? (molar mass * moles = mass)

so go ahead and solve for x, the constant by which the formula CHF is multiplied by to find the molecular formula.

Hope this helps! If a specific part was confusing, please copy it so I can explain better.