Gas Law and Heating/Cooling Curve Practice - WS 1 5.00 g of oxygen gas, 4.00 g o
ID: 477828 • Letter: G
Question
Gas Law and Heating/Cooling Curve Practice - WS 1 5.00 g of oxygen gas, 4.00 g of neon gas, and 6.25 g of fluorine gas are added to a 0.0248 kL container at 31.0 degree C. a. Determine the partial pressure in atm of each gas present. b. Determine the total pressure in atm of the gas present. c. Determine the percent by mass of neon gas in the container, (not on the next test) d. Determine the mole fraction of fluorine gas in the container, (not on the next test) Aluminum metal reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. a. Write and balance the reaction. What kind of reaction is this? b. If 25.0 g of Al reacts with 40.0 g of 11C1, then determine the limiting reactant. c. Determine the moles of hydrogen gas produced. d. If the hydrogen gas is collected in a 10.0-gallon container at a pressure of 795 mmHg. then determine the temperature of the gas in degree C.Explanation / Answer
1. firstly, let us calculate number of moles of each gas
number of moles of O2 = nO2 = 5/16 = 0.3125 moles
number of moles of Ne = nNe = 4/20.18 = 0.198 moles
number of moles of F = nF = 6.25/19 = 0.329 moles
a) partial pressures of each gas is
pO2 = nRT/V =(0.3125 x 0.08206 x 304) / (24.8L) = 0.314atm
pNe = (0.198 x 0.08206 x 304) / (24.8L) = 0.199atm
pF = (0.329 x 0.08206 x 304) / (24.8L) = 0.331atm
b) Total pressure of gases present is
P = pO2 + pNe + pF = 0.314+0.199+0.331 = 0.844atm
c) Percent by mass of Neon gas is
Mass percent of neon =( mass of neon in grams / total mass in grams ) x 100
= (4/15.25) x 100
= 26.23%
d) mole fraction of Fluorine is
XF = mass of F in moles / total mass in moles
= 0.329 / 0.8395
= 0.3919.
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