A compound has the empirical formula SF_4. At 20.0 degree C, 0.100 g of the gase

Question

A compound has the empirical formula SF_4. At 20.0 degree C, 0.100 g of the gaseous compound occupies a volume of 22.1 mL and exerts a pressure of 1.02 atm. What is the molecular formula of the gas? Methane (CH_4) reacts with oxygen gas to produce carbon dioxide gas and liquid water. If 15.0 moles of methane react, what is the volume of the carbon dioxide (in liters) produced at 23.0 degree C and 0.985 atm? In alcohol fermentation yeast converts glucose to ethanol and carbon dioxide: C_6 H_12 O_6 (s) rightarrow 2C_2 H_5 OH(l) + 2CO_2(g) If 5.97 g of glucose reacts and 1.44 L of CO_2 gas is collected at 293 K and 0.984 atm, what was the percent yield of the reaction?

Explanation / Answer

4)

Temperature = 20 C = 293 K

Mass = 0.1 g

Volume = 22.1 ml = 0.0221 L

Pressure = 1.02 atm

R = 0.08206 L.atm/mol.K

P * V = n * R T

1.02 atm * 0.0221 L = n * 0.08206 L.atm/mol.K * 293 K

n = 9.375 * 10-4 moles

Molar mass = mass / no. of moles = 0.1 g / 9.375 * 10-4 moles = 106.7 g/mol

Molar mass calculated from emprical formula = 108 g/mol

ratio between these molar mass is almost equal to 1

so emprical formula and molecular formula will be same

Molecular formula will be SF4

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