Molecular formula?

Question

Calculate the molecular formula of Arsenic sulfide when it is in the gaseous state (volume 60.5cm3 and mass 0.345) at 650C (3 sig Calculate the molecular figures)

Show reasoning.

Also show the molecular formula at 1573C (3 sig figures)( volume 0.345 and mass 242.0) I need a short setence to show how you came to the conclusion.

Answer 1

Is it AS2S4 you had in mind?
Or are referring to the number of moles?

From ideal gas law
PV=NkT
P- pressure
V- volume
k - Boltzmann’s const - (1.381 E−23 joule/Kelvin )
N- Number of molecules
T- Temperature in deg K

N0=a mole is 6.022 E+ 23 molecules
Moles = m/(gm moles)
Moles of AS2S4 =( 74.92) 2 +( 32.07)4=278 gm moles

N= Moles N0 =
N=(0.345 gm /278 gm moles) x 6.022 E+23 molec/moles)
N=747 334 532 374 100 719 424 = 747 E+18 molecules

The answer is proportional to the question