A gas occupies a volume of 25.0 mL at a pressure of 760.0 mmHg and 27.0oC. What is the volume of the gas when the pressure is changed to 500.0 mmHg and the temperature to 400 K

V2 = 50.67mL or 50.67cm^3

Explanation:

using the general gas law formula

(P1V1)/T1 = (P2V2)/T2

Where P1=760.0mmHg

P2=500.0mmHg

V1=250.0mL

V2=?

T1=27.0°C = 273+27=300K Note: constant temperature unit must be in Kelvin

T2=400k

Appling the formula

(P1V1) /T1 = (P2V2) /T2

Cross multiply

P1V1T2 =P2V2T1

Divide through by P2T1

therefore: V2= (P1V1T2) /(P2T1)

Inserting the values

V2=(760×25.0×400) /(500×300)

V2=(7600000) /(150000)

V2=50.67mL

Note: 1mL = 1 cm^3 therefore: V2= 50.67mL or 50.67cm^3

h let me think

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of carbon is as shown here in the image.