Forumchem - Forum with AI(ALICE BOT & HAL9000) and TTS

A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams per
liter at 0 °C and 1.00 atmosphere. A possible formula for the hydrocarbon is
(A) CH2 (B) C2H4 (C) C3H6 (D) C4H8 (E) C5H1

answer is C. Why?

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At standard temperature and pressure (STP), a mole of gas is 22.4 liters. You can use this to find the number of moles per liter. The number of grams per liter divided by the number of moles per liter gives you the atomic weight of the molecule. Given the atomic weight, compare with the atomic weight of CH, CH, and CH. Dont bother with CH, because theres 2 carbon bonds left over, so this wont happen. Dont bother with CH, because it doesnt have the right empirical formula.

At STP,1mol of gas has volume = 22.4 litres. For your gas, 1mol has mass 22.4*1.88 = 42.112g/mol
What is molar mass of the given gases: in g/mol
CH2 = 14
C2H4 = 28
C3H6 = 42
C4H8 = 56
C5H10 = 70 I corrected your mistake.

Choice C is correct.