A quantity of gas occupies a volume of 506 cm 3 at a temperature of 147 o C.
Assuming the pressure stays constant, at what temperature will the
volume of the gas be 604 cm 3 ?

228.3°C

Explanation:

Data obtained from the question include:

V1 (initial volume) = 506 cm3

T1 (initial temperature) = 147°C = 247 + 273 = 420K

V2 (final volume) = 604 cm3

T2 (final temperature) =?

The gas is simply obeying Charles' law because the pressure is constant.

The final temperature of the gas can be obtained by using the Charles' law equation V1/T1 = V2/T2 This is illustrated below:

V1/T1 = V2/T2

506/420 = 604/T2

Cross multiply to express in linear form as shown:

506 x T2 = 420 x 604

Divide both side by 506

T2 = (420 x 604) /506

T2 = 501.3K

Now let us convert 501.3K to a temperature in celsius scale. This is illustrated below:

°C = K - 273

°C = 501.3 - 273

°C = 228.3°C

Therefore, the temperature of the gas when the volume of the gas is 604 cm3 is 228.3°C

it should be all of them because it asks if you included all of those in your answer

explanation:

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be