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Alexxandr [17]
2 years ago
10

A sample of n2 gas occupies 2.40 l at 20°c. if the gas is in a container that can contract or expand at constant pressure, at wh

at temperature will the n2 occupy 4.80 l?
Chemistry
2 answers:
dolphi86 [110]2 years ago
8 0

<u>Answer:</u> The final temperature of the gas comes out to be 313°C

<u>Explanation:</u>

To calculate the final temperature of the gas, we use the equation given by Charles' Law. This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

\frac{V_1}{T_1}=\frac{V_2}{T_2}

where,

V_1\text{ and }T_1 are the initial volume and temperature of the gas.

V_2\text{ and }T_2 are the final volume and temperature of the gas.

We are given:

V_1=2.40L\\T_1=20^oC=(20+273)K=293K\\V_2=4.80L\\T_2=?

Putting values in above equation, we get:

\frac{2.40L}{293K}=\frac{4.80L}{T_2}\\\\T_2=\frac{4.80\times 293}{2.40}=586K

Converting the temperature from kelvins to degree Celsius, by using the conversion factor:

T(K)=T(^oC)+273

586=T(^oC)+273\\T(^oC)=313^oC

Hence, the final temperature of the system comes out to be 313°C

Bas_tet [7]2 years ago
4 0
From Charle's law the volume of a fixed mass of a gas is directly proportional to the absolute temperature at constant pressure.
Therefore';
V1/T1=V2/T2
    Where; V1 = 2.40 l, T1 = 273 +20= 293 K, V2 = 4.80, and T2= ?
 2.4/293= 4.8/T2
 T2= (4.8×293)/2.4
       = 586 K or  313° C
     

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<u>So, the right answer is</u>

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