Question

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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?

Answer 1

Answer:

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

Answer 2

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:-

• Pressure
• Temperature
• Volume

Hence the formula we gonna use is as follows:-

$PV = nRT$

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

Hence it is equal to

$\frac{PV}{T} = \frac{PV}{T}$

Put the value given,

$\frac{80*50}{273} = \frac{1880*39}{T}$

Solving the equation, the value T will be:-

$T2 = \frac{20016360}{44000}$

=181.92C

The temperature given is 181.92C

For more information, refer to the link:-

https://brainly.com/question/1437490