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belka [17]
3 years ago
14

A sample of a gas (1.50 mol) is contained in a 15.0 l cylinder. the temperature is increased from 100 °c to 150 °c. what is the

ratio of final pressure to initial pressure?
Chemistry
1 answer:
pav-90 [236]3 years ago
7 0

<u>Given:</u>

Moles of gas, n = 1.50 moles

Volume of cylinder, V = 15.0 L

Initial temperature, T1 = 100 C = (100 + 273)K = 373 K

Final temperature, T2 = 150 C = (150+273)K = 423 K

<u>To determine:</u>

The pressure ratio

<u>Explanation:</u>

Based on ideal gas law:

PV = nRT

P= pressure; V = volume; n = moles; R = gas constant and T = temperature

under constant n and V we have:

P/T = constant

(or) P1/P2 = T1/T2 ---------------Gay Lussac's law

where P1 and P2 are the initial and final pressures respectively

substituting for T1 and T2 we get:

P1/P2 = 373/423 = 0.882

Thus, the ratio of P2/P1 = 1.13

Ans: The pressure ratio is 1.13


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Explanation:

The electron is jumped into higher level and back into lower level by absorbing and releasing the energy.

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When the energy is provided to the atom the electrons by absorbing the energy jump to the higher energy levels. This process is called excitation. The amount of energy absorbed by the electron is exactly equal to the energy difference of orbits.  For example if electron jumped from K to L it must absorbed the energy which is equal the energy difference of these two level. The excited electron thus move back to lower energy level which is K by releasing the energy because electron can not stay longer in higher energy level and comes to ground state.

De-excitation:

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