A 1.00 mol of helium, He gas fills up an empty balloon to a volume of 1.50 L. Calculate the volume of the balloon if an additional 2.50 mol of He gas is added. The temperature and pressure of the gas are constant. 1
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.
![A 1.00 mol of helium, He gas fills up an empty balloon to a volume of 1.50 L.
Calculate the volume of the balloon if an additional 2.50 mol of He gas is added. The
temperature and pressure of the gas are constant.
1
[2]
A 4.00 L of methane, CH4 is burned in excess oxygen at 25.0 °C and 1.50 atm to
produce water and carbon dioxide.
2
CH4 (g) + 2 02(g) → CO2(g) + 2 H20(1)
Calculate the volume of carbon dioxide produced after the reaction has stopped.
[Assume the temperature and pressure of product are the same with reactant.
[6]
R=0.0821
atm. LmolK1]
3
(a)
State Dalton's Law.
[1]
(b) A 90.0 mL of neon, Ne at 27.0 °C and 5.00 atm is mixed with nitrogen, N2 and
transferred into a 200.0 mL container at the same temperature. The total pressure
of the mixture is 4.25 atm. Calculate the partial pressure of Ne and N2.
[4]
4
State two basic assumptions of kinetic molecular theory of gasses. [2]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3431989a-830e-48de-8ba8-a0b72b8ae9b2%2F04960091-6015-4623-867b-4d2c39622fd0%2Fnxym6j8_processed.jpeg&w=3840&q=75)
![For the reaction X + Y → 2Z, the following data were obtained:
Experiment
[X] (M)
[Y] (M)
Initial Rate (M/s)
8.00 x 10-4
8.00 x 10-4
5.90 x 10-3
1.20 x 10-2
5.60 x 10-8
2.24 x 10-7
1
3
1.60 x 10-3
5.90 x 10-3
1.10 x 10-7
4
2.30 x 10-3
1.30 x 10-2
8.90 х 10-7
(a)
Based on the data above, calculate the rate law.
[6]
(b)
Calculate the rate constant of the reaction using experiment 1.
[3]
The rate constant for decomposition of N205 is 6.2 x 10-4 min-1. Calculate the time it takes
for the concentration of N205 to decrease to 16.5% from its initial concentration. The
initial concentration of N2Os is 1.00 M.
[2]
7 State two criteria for a proposed mechanism to be a valid.
[2]
8
Given the following reaction mechanism:
[2]
Step 1: NO2CI (g) → NO2 (g) + CI (g)
Step 2: NO2CI (g) + CI (g)
(slow)
(fast)
→ NO2 (g) + Cl2 (g)
(a)
Write the rate law for the rate determining step.
[1]
(b)
Identify the intermediate for the reactions above.
[1]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3431989a-830e-48de-8ba8-a0b72b8ae9b2%2F04960091-6015-4623-867b-4d2c39622fd0%2Fiwuxxvj_processed.jpeg&w=3840&q=75)
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