Question

At 20°C a confined ammonia gas has a pressure of 2.50 atm.At what temperature would its pressure be equal to 760 mmHg answer.

Answer 1

Hello!

At 20°C a confined ammonia gas has a pressure of 2.50 atm, at what temperature would its pressure be equal to 760 mmhg ?

Note: Charles' Law and Gay-Lussac's Law should be in Kelvin (absolute temperature).

We have the following information:

T1 (initial temperature) = 20 ºC (in Kelvin)

TK = TC+273.15 → TK = 20+273.15 → TK = 293.15

T1 (initial temperature) = 293.15 K

P1 (initial pressure) = 2.50 atm

T2 (final temperature) = ? (in Kelvin)

P2 (final pressure) = 760 mmHg → P2 (final pressure) = 1 atm

According to the Law of Charles and Gay-Lussac in the study of gases, we have an isochoric (or isovolumetric) transformation when its volume remains constant or equal. If the pressure decreases, its temperature will also decrease. (directly proportional to pressure with temperature), then we have the following formula:

$\dfrac{P_1}{T_1} = \dfrac{P_2}{T_2}$

$\dfrac{2.50}{293.15} = \dfrac{1}{T_2}$

multiply the means by the extremes  

$2.50*T_2 = 293.15*1$

$2.50\:T_2 = 293.15$

$T_2 = \dfrac{293.15}{2.50}$

$\boxed{\boxed{T_2 = 117.26\:K}}\:\:\:\:\:\:\bf\green{\checkmark}$

Answer:  

The temperature is 117.26 K  

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I Hope this helps, greetings ... Dexteright02! =)

Answer 2

Answer:

TF=117.16K

Explanation:

concept - Gay-lussac's law , pressure is directly proportional to the temperature when volume remains constant .

pi/Ti= pf/TF

given - pi= 2.50atm

Ti= 20°C= 20+273.15=293.15K

pf= 760mmHg= 1atm

find- TF=?

explanation-

pi/Ti= pf/TF

2.50/293.15=1/TF

TF=293.15/2.5

TF=117.16K

Temperature at which pressure is equal to 760mm Hg is 117.16K

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