4. a student is doing experiments with co2(q) . originally a sample of the gas is in a rigid container at 299 kand 0.70 atm. the student increases the temperature of the co2(g) ) in the container to 425 k the co2(g)mo molecul (b) calculate the pressure of the co - (g) ) in the container at 425 k (c) in terms of kinetic molecular theory, briefly explain why the pressure of the co2(g) in the container changes as it is heated to 425 k. (d) the student measures the actual pressure of the co2(g) in the container at 425 k and observes that it is less than the pressure predicted by the ideal gas law . explain this observation ,

b. 0,99atm

c. Answer is in the explanation

d. Answer is in the explanation

Explanation:

b. Using Gay-Lussac's law:

P₁T₂ = P₂T₁

P₁: 0,70 atm; T₂: 425K; P₂: ??; T₁: 299K

0,70atm×425K / 299K = 0,99 atm

c. Using kinetic molecular theory, the increasing of temperature increases the kinetic energy of gas particles and if kinetic energy increases, the pressure increases. That means the increasing of temperature increases the pressure in the system.

d. Now, the increases in kinetic energy of gases increase the collisions betwen particles. As these intermolecular forces that are not taken into account in ideal gas law, the observed pressure will be different to the pressure predicted by ideal gas law.

I hope it helps!

The pressure of the gas increases from 0.70 atm to 0.99 atm as the temperature is increased. The interaction of the gas molecules causes the pressure of the gas to deviate from the predicted value.

From the information in the question;

Initial temperature(T1) =  299 K

Initial pressure (P1) = 0.70 atm

Final pressure (P2) = ?

Final temperature (T2) = 425 K

Given that;

P1/T1 = P2/T2

P1T2 = P2T1

P2 = P1T2/T1

P2 = 0.70 atm × 425 K/ 299 K

P2 = 0.99 atm

In terms of the kinetic molecular theory, we know that the pressure of a gas has to do with its bombardment of the walls of the container. When the temperature of the gas is increased, the gas molecules become more energetic and bombard the walls of the container more frequently hence the pressure of the gas increases.

The particles of an ideal gas do not to interact with each other according to theory. However, real gases molecules interact with each other. Hence, actual pressure of the CO2(g) in the container at 425 K is less than the pressure predicted by the ideal gas law. More significant particle interaction decreases the pressure of the gas compared the value predicted based on the ideal gas law.

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