No hand written answers A 2.10-L vessel contains 4.65 g of a gas at 1.00 atm and

Question

No hand written answers

A 2.10-L vessel contains 4.65 g of a gas at 1.00 atm and 27.0°C. (a) Calculate the density of the gas in grams per liter. (b) What is the molar mass of the gas? (10 points)

(Reference: Chang 5.47)

A certain anesthetic contains 64.9 percent carbon, 13.5 percent hydrogen, and 21.6 percent oxygen by mass. At 120°C and 750 mmHg, 1.00 L of the gaseous compound weighs 6.90 g. What is the molecular formula of the compound? (10 points)

What is the mass of the solid NH4Cl formed when 73.0 g of NH3(g) are mixed with an equal mass of gaseous HCl? What is the volume and identity of the gas remaining, measured at 14.0°C and 752 mmHg? (8 points)

        NH3(g) + HCl(g) NH4Cl

(Reference: Chang 5.59)

A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The total pressure is 1.50 atm. Calculate the partial pressures of the gases. (8 points)

(Reference: Chang 5.67)

Explanation / Answer

Question 1.

A 2.10-L vessel contains 4.65 g of a gas at 1.00 atm and 27.0°C.

(a) Calculate the density of the gas in grams per liter.

D = mass/Volume

D = 4.65 / 2.10

D = 2.21428 g/L

(b) What is the molar mass of the gas? (10 points)

PV = nRT

n = mass/MW , and D = mass/V; substitute in ideal gas laws

D = P*MW/(RT)

solve for MW

MW = D*RT/P

MW = (2.21428 )(0.082*300) / 1

MW = 54.471 g/mol

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