If a 600.0 mL volume of a sample gas has a mass of 1.60 g t 2.00 atm and 27.00 d

Question

If a 600.0 mL volume of a sample gas has a mass of 1.60 g t 2.00 atm and 27.00 degree C, which of the following gases could it be? NH_3 O_2 SO_2 Kr When 7.50 g of zinc metal reacts with excess HCI, how many liters of H_2 gas can form at STP? 0.114 L 0.229 L 2.57 L 5.15 L Diethyl ether has a boiling point of 34.5 degree C and 1-butanol has a boiling point of 117 degree C. Both compounds have the same molecular weight and same molecular formula (C_4H_10O). Which statement best explains the difference in boiling points? The strength of London dispersion forces is greater in 1-butanol Oxygen is toward the end of the structure in 1-butanol and in the middle of the structure in Diethyl ether The 1-butanol molecules can form strong hydrogen bonds with other 1-butanol molecules. Diethyl ether forms dipole-dipole intermolecular forces, which are not as strong as hydrogen bonds The Diethyl ether molecules have more hydrogen atoms in place to form strong hydrogen bonds with other Diethyl ether molecules. 1-butanol also forms hydrogen bonds, but not as many as Diethyl ether.

Explanation / Answer

Question 31.

V = 600 mL = 0.6 L

m = 1.6 g

P = 2 atm

T = 27°C = 27+273 = 300 K

R = 0.082 Latm/molK

first, find moles so we can relate mass to moles

apply ideal gas law

PV = nRT

n = PV/(RT)

n = 2*0.6/(0.082*300) = 0.04878048 moles

then

MM = mass of gas / moles of gas = 1.6/0.04878048 = 32.8 g /mol

best fit is O2, with MW = 32 g/mol

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