Question 3.

What is an ideal gas.

When 17.75 g of Cl2 gas filled into a 3-L closed container at 27 °C, the internal pressure of the container increased to 1.6 atm. Determine whether Cl2 gas behaves as an ideal gas at this condition. State the conditions whaen a gas deviates from an ideal behaviour. Explain your answer.

 

Question 4.

The decomposition of KClO3 is commonly used to prepare small amounts of O2 in the laboratory. Oxygen gas generated in an experiment is collected at 25 °C in a bottle inverted in a breaker of water. The external laboratory pressure is 762 torr. When the water level in the originally full bottle has fallen to the level in the breaker, the volume of collected gas is 1750 mL. What is the mass of oxygen gas have been collected?

[vapour pressure of water at 25 °C = 23.8 torr]

 

question 3

Answer:

Step-by-step explanation:

gas behaves more like an ideal gas at higher temperature and lower pressure, as the potential energy due to intermolecular forces becomes less significant compared with the particle's kinetic energy, and the size of the molecules becomes less significant.

Here, the pressure increases it means there is the interaction between the molecules and if interaction is there means they are not behave like ideal gas.

Any gas deviates from its ideal behaviour at loe temp and high pressure. In this condition the volume of the particles is not negligible as compared to the volume of the gas 

. also the intermolecular force starts acting upon the molecules. Hence gas doesn't  behave ideally.

Answer:

Step-by-step explanation:

The input force is 50 N. But it will not create not any change. No mechanical advantage is observed.

Answer:

Step-by-step explanation:

It is clear by the equation 2(27+3×35.5)= 267 gm of AlCl3 reacts with 6× 80 = 480 gm of Br2 . So 29.2 gm reacts = 480× 29.2/267= 52.6 gm

Calcium (Ca)(On the periodic table, ionization energy increases as you go up and to the right of the periodic table)

Answer:

Taking into accoun the ideal gas law, The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L.

An ideal gas is a theoretical gas that is considered to be composed of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:  

P×V = n×R×T

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas. The universal constant of ideal gases R has the same value for all gaseous substances.

Explanation:

In this case, you know:

P= 0.884 atm

V= ?

n= 0.857 moles (where 28 g/mole is the molar mass of N₂, that is, the amount of mass that the substance contains in one mole.)

R=0.082

T= 328 K

Replacing in the ideal gas law:

0.884 atm×V= 0.857 moles× 0.082 ×328 K

Solving:

V= 26.07 L

The volume of a container that contains 24.0 grams of N2 gas at 328K and 0.884 atm is 26.07 L.