Urgent!! SOMEONE PLEASE HELP THANK YOU! A gas occupies a volume of 555 mL at 0 °C and 8 0.0 kPa. What is the final celsius temperature when the volume of the gas is changed to 1880 mL and the pressure is changed to 39 kPa?

The ideal gas law, also called the general gas equation, is the equation of the state of a hypothetical ideal gas.

The ideal gas law work under the constant:-

Hence the formula we gonna use is as follows:-

In the question, the pressure, temperature, and volume are given in two different system

Hence it is equal to

Put the value given,

Solving the equation, the value T will be:-

=181.92C

The temperature given is 181.92C

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The final temperature is 181.92°C

Explanation:

Given

Initial Temperature, T1 = 0°C

Initial Volume, V1 = 555mL

Initial Pressure, P1 = 80.0kPa

Final Volume, V2 = 1880ml

Final Pressure, P2 = 39kPa

Required

Determine the Final Temperature, T1

This question illustrates ideal gas law and will be solved using:

(P1 * V1)/T1 = (P2 * V2)/T2

But first, we need to convert temperature to degree Kelvin

T1 = 0°C = 273 + 0 = 273k

Next, we substitute values for P1, V1, T1, P2 and V2

THE EQUATION BEFOMES

(80 * 550)/273 = (1880 * 39)/T2

44000/273 = 73320/T2

Cross Multiply

44000 * T2 = 73320 * 273

44000T2 = 20016360

Solve for T2

T2 = 20016360/44000

T2 = 454.92K

Convert to degree Celsius

T2 = 454.92 - 273

T2 = 181.92°C

Hence, the final temperature is 181.92°C

3 hours because it is a decent distance.