Acompound is composed of 85.64% carbon and 14.36% hydrogen. the compound has a formula mass of 42.08 grams. what is the molecular formula?

Explanation:

1) Assume 100 g of substace:

2) Convert the masses in grams to number of moles

Calculations:

3) State the ratio of moles.

Divide the number of moles of each element by the least number of moles:

4) Set the empirical formula:

5) Calculate the mass of one mol of the empirical formula:

6) Calculate how many times the mass of the empirical formula is contained in the mass of the molecular formula:

7) Set the molecular formula:

Multiply each subscript of the empirical formula by the previos ratio: 3

Conclusion: the molecular formula is C₃H₆

C₃H₆

Explanation:

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

it is a good conductor

explanation: