So I'm a little stuck on two questions, firstly I calculated the empirical formula of a compound which was C2H4Cl and now I need to find the molecular formula so I did the relative empirical mass (89.3) then divided the actual formula mass (127) but that gave me 1.422172452 so I'm confused as to what to scale up by, just 1 so it stays the same?
Next question is the same but the empirical formula so far is 1, 3 and 1.34, so should I multiply them all by 3 to get 3, 6 and 4?
So I'm a little stuck on two questions, firstly I calculated the empirical formula of a compound which was C2H4Cl and now I need to find the molecular formula so I did the relative empirical mass (89.3) then divided the actual formula mass (127) but that gave me 1.422172452 so I'm confused as to what to scale up by, just 1 so it stays the same?
Next question is the same but the empirical formula so far is 1, 3 and 1.34, so should I multiply them all by 3 to get 3, 6 and 4?
Thanks!
It would be a lot more helpful and easier if you upload the Q, so we can see where you went wrong
It would be a lot more helpful and easier if you upload the Q, so we can see where you went wrong
Hahaa okay, sorry here it is
1) A halogenoalkene, H, has relative formula mass 127 and the following comp by mass: C:37.8% H:6.3% Cl:55.9% Show that the empirical formula oh H is C2H4Cl (Which I did okay)
Then deduce molecular mass.
Thanks!
**EDIT** The second one's okay now, I divdied by 12 instead of 16 for O, sorry! Just number 1
1) A halogenoalkene, H, has relative formula mass 127 and the following comp by mass: C:37.8% H:6.3% Cl:55.9% Show that the empirical formula oh H is C2H4Cl (Which I did okay)
Then deduce molecular mass.
Thanks!
**EDIT** The second one's okay now, I didividedy 12 instead of 16 for O, sorry! Just number 1
So you did N=Mass/M for all of them? 37.8/12=x Did you then divide it by the smallest and get ratios? I hope I am right, as I am a bit rusty -_-