A0.02877 g sample of gas occupies 10.0-ml at 289.0 k and 1.10 atm. upon further analysis, the compound is found to be 38.734% c and 61.266% f. what is the molecular formula of the compound? (order: c, x)

Assuming ideal gas, we calculate the number of moles.

PV = nRT

n = PV / RT

n = (1.10 atm) (10 x 10^-3L) / [(0.08205746 L atm / mol K) (289 K)]

n = 4.64 x 10^-4 mol

SO the molar mass is:

molar mass = 0.02877 grams / 4.64 x 10^-4 mol

molar mass = 62.02 g/mol

The only possible combination is:

C2F2

C = 12 * 2 = 24

F = 19 * 2 = 38

24 + 38 = 62 g/mol

i think it is d. e because the next one is igneous.

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.