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A gas compound is 78.14 percent boron and 21.86 percent hydrogen At 27C 74.3 ml of the gas exerted a pressure of 1.12 ATM If the mass of the gas was 0.0934 g what is its molecular formula?
Wiki User
∙ 14y ago
v = 0.0743 l
t = 27 + 273 = 300 k
n = pv / rt = 1.12 x 0.0743 / 0.0821 x 300 = 0.00338
molar mass = 0.0934 / 0.00338 = 27.6 g/mol
78.14 / 10.811 = 7.22
21.86 / 1.00794 = 21.69
We divide by smallest number :
7.22 / 7.22 = 1 (boron)
21.69 / 7.22 = 3 ( hydrogen)
b1h3 is the empirical formula
mass empirical formula = 13.8
27.6 / 13.8 =2
The molecular formula is b2h6.
Wiki User
∙ 14y ago
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