Reference no: EM132409914
1. If you place 10.0 L of methanol (CH4O) in a sealed room that is 4.75 m long, 2.5 m wide, and 2.5 m high, will all the methanol evaporate? If some liquid remains, how much will there be? The vapor pressure of methanol is 127 torr at 25 °C, and the density of the liquid at this temperature is 0.791 g/mL. Treat the room dimensions as exact numbers.
2. Ethylene burns in oxygen according to the following equation:
C2H4 + 3 O2 → 2 CO2 + 2 H2O
(a) How many liters of O2 at 30 °C and 0.214 atm will be needed to burn 5.92 L of C2H4 at 30 °C and 0.214 atm?
(b) How many liters of CO2 at 30 °C and 0.214 atm will be produced? Report your answers to parts (a) and (b) to 3 significant figures.
3. Complete combustion of a 0.0150 mol sample of a hydrocarbon, CxHy, gives 1.008 L of CO2 at STP and 0.540 g of H2O.
(a) What is the molecular formula of the hydrocarbon?
(b) What is the empirical formula of the hydrocarbon?
4. What is the molar mass of a compound if a gaseous sample has a density of 3.140 g/L at 30 °C and 491 torr? The temperature in Celsius is known to two significant figures.
5. A 0.500-L bulb containing He at 330 torr is connected by a valve to a 1.00-L bulb containing CO2 at 210 torr. The valve between the two bulbs is opened and the two gases mix. The initial gas pressures as known to three significant figures.
(a) What is the partial pressure (torr) of He?
(b) What is the partial pressure (torr) of CO2?
(c) What is the total pressure?
(d) What is the mole fraction of He?
6.Consider the following entities: Ar, SiH3F, Xe, and CClF3.
(a) Which one will diffuse the fastest?
(b) What is the rms speed (m/s) of the slowest-moving atom or molecule at 25°C?
7.You are given 2.078 g of a mixture of KClO3 and KCl. When heated, the KClO3 decomposes to KCl and O2, 2KClO3 (s) → 2KCl (s) + 3O2 (g), and 338 mL of O2 is collected over water at 27 °C. The total pressure of the gases in the collection flask is 762 torr. What is the weight percentage of KClO3 in the sample?
The formula weight of KClO3 is 122.55 g/mol. The vapor pressure of water at 27 °C is 26.7 torr.
8. The compound CO has van der Waals constants a = 1.472 atm•L2/mol2 and b = 0.0395 L/mol. Using both the ideal gas law and van der Waals's equation, calculate the pressure expected for 12 mol of CO gas in a 4.00-L container at 0 °C.
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: The vapor pressure of methanol is 127 torr at 25 °C, and the density of the liquid at this temperature is 0.791 g/mL. Treat the room dimensions as exact numbers
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