3. (77, 87, 133) The complete combustion of ethanol is performed according to the reaction given below in a sealed rigid 450.OL container. Before the reaction begins the pressure is 2.3atm and the temperature is 298K. At the conclusion of the reaction the pressure is 3.1atm and the temperature is maintained at 298K C2H;OH(1) + 302(g) → 2CO2(g) + 3H20(g) a. Which species is the limiting reactant? b. At the end of the reaction which gas species are present? c. Calculate the partial pressure, in atm, of each gas present at the end of the reaction. d. What mass, in g, of ethanol was consumed? e. Provide a ranking of the rate of effusion from slowest to fastest for the three gases. 4. (91) 175.0g of methane (CHa) is held in a 35.0L container at 195K. a. Calculate the real pressure of the gas, in atm, using the van der Waals values given in Table 10.4. Report with 5 significant figures. b. Calculate the ideal pressure of the gas, in atm. Report with 5 significant figures. Do repulsive or attractive forces dominate in the sample? C. 5. (57,71,105) An unknown compound (A) is decomposed according to the reaction given below. One of the gas identities is also unknown and represented as Y. The gases are collected over water at 290K. The final volume of the gas sample is 565mL and the pressure is 750torr. At 290K the vapor pressure of water is 14.53torr. 2A(1) → 2Y(g) + 02(g) a. Calculate the total number of moles of gas that were produced in the reaction. b. Calculate the partial pressures of each of the gases, in atm. The density of the gas sample (without the water included) is 2.06 g/L. What is the molar mass, in g/mol, of the unknown gas, Y? d. How many moles of A were consumed in the reaction? C.
3. (77, 87, 133) The complete combustion of ethanol is performed according to the reaction given below in a sealed rigid 450.OL container. Before the reaction begins the pressure is 2.3atm and the temperature is 298K. At the conclusion of the reaction the pressure is 3.1atm and the temperature is maintained at 298K C2H;OH(1) + 302(g) → 2CO2(g) + 3H20(g) a. Which species is the limiting reactant? b. At the end of the reaction which gas species are present? c. Calculate the partial pressure, in atm, of each gas present at the end of the reaction. d. What mass, in g, of ethanol was consumed? e. Provide a ranking of the rate of effusion from slowest to fastest for the three gases. 4. (91) 175.0g of methane (CHa) is held in a 35.0L container at 195K. a. Calculate the real pressure of the gas, in atm, using the van der Waals values given in Table 10.4. Report with 5 significant figures. b. Calculate the ideal pressure of the gas, in atm. Report with 5 significant figures. Do repulsive or attractive forces dominate in the sample? C. 5. (57,71,105) An unknown compound (A) is decomposed according to the reaction given below. One of the gas identities is also unknown and represented as Y. The gases are collected over water at 290K. The final volume of the gas sample is 565mL and the pressure is 750torr. At 290K the vapor pressure of water is 14.53torr. 2A(1) → 2Y(g) + 02(g) a. Calculate the total number of moles of gas that were produced in the reaction. b. Calculate the partial pressures of each of the gases, in atm. The density of the gas sample (without the water included) is 2.06 g/L. What is the molar mass, in g/mol, of the unknown gas, Y? d. How many moles of A were consumed in the reaction? C.
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Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
Question
Transcribed Image Text:3. (77, 87, 133) The complete combustion of ethanol is performed according to the reaction given below in a
sealed rigid 450.0L container. Before the reaction begins the pressure is 2.3atm and the temperature is 298K.
At the conclusion of the reaction the pressure is 3.1atm and the temperature is maintained at 298K
C,H5OH(1) + 302(g) → 2CO2(g) + 3H20(g)
a. Which species is the limiting reactant?
b. At the end of the reaction which gas species are present?
c. Calculate the partial pressure, in atm, of each gas present at the end of the reaction.
d. What mass, in g, of ethanol was consumed?
e. Provide a ranking of the rate of effusion from slowest to fastest for the three gases.
4. (91) 175.0g of methane (CH4) is held in a 35.0L container at 195K.
a. Calculate the real pressure of the gas, in atm, using the van der Waals values given in Table 10.4. Report
with 5 significant figures.
b. Calculate the ideal pressure of the gas, in atm. Report with 5 significant figures.
c. Do repulsive or attractive forces dominate in the sample?
5. (57,71,105) An unknown compound (A) is decomposed according to the reaction given below. One of the gas
identities is also unknown and represented as Y. The gases are collected over water at 290K. The final volume
of the gas sample is 565mL and the pressure is 750torr. At 290K the vapor pressure of water is 14.53torr.
2A(1) → 2Y(g) + 02(g)
a. Calculate the total number of moles of gas that were produced in the reaction.
b. Calculate the partial pressures of each of the gases, in atm.
The density of the gas sample (without the water included) is 2.06 g/L. What is the molar mass, in
g/mol, of the unknown gas, Y?
C.
d. How many moles of A were consumed in the reaction?
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