What is the molecular formula for 40.0%C, 6.6%H, and 53.4%H ; molar mass = 120g?

Question

CHEMiSTRY

Answer 1

.40 * 120g = 48 g C
.066 * 120g = 7.92 g H
.534 * 120g = 64.08 g O .... (i'm assuming that last one is Oxygen)

C4H8O4 should be your molecular formula

Answer 2

You have to percentages for H, I think one is supposed to be something else. Probably O?

So if it was 40% C (MW=12) 6.6% h (MW=1) and 53.4% )O, (MW=16).
of 120 g, 40% is C, so that is .4 * 120 = 48 G of C (48/12=4 atoms)
.066 * 120 = 8 grams of H (8/1=8 atoms)
.53 * 120 = 63.6 g O, which is 63.6/16 = 4 atoms.

so C4 H8 O4

Answer 3

masses of the componentsin100g=.C=40g;H=6.6
O=53.4g
molecular formula weight/molar mass=120g
the formula=C4H8O4
C=(120*40)/(100*12)=4 H=(120*6.6)/(100*1)=8
O=(120*53.4)/(100*16)=4

Answer 4

I take it those are possibilities by skill of mass. assume you're taking one hundred gram of those issues, then 40 grams is C, 6.6 grams is H and fifty 4.4 grams is O. replacing to mols this can provide you 40/12.01=3.33 mol C, 6.6/one million.01= 6.fifty 3 mol H, fifty 4.4/16=3.4 mol O, dividing all by skill of the smallest decision 3.33 provides you one million mol C, one million.ninety six= 2 mol H, one million mol O This shows that the empirical formulation for the compound is CH2O The molar mass of this compound is about 30. because the genuine molar mass is 120, we ought to multiply all by skill of a area 4. therefore the genuine molecular formulation is C4H8O4

Answer 5

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