The pressure exerted on a sample of gas is 735 mm hg with a volume of 375 ml and a temperature of 25 degrees celsius. what would the pressure of the gas be if the temperature was reduced to standard temperature and the volume was expanded to 500.0 ml?

= 498.13 mmHg

Explanation:

Using the combined gas law;

P1V1/T1 =P2V2/T2

in this case; P1 = 725 mmHg, V1 = 375 mL and T1 = 25°C + 273 = 298 K

P2 = ?  V2 = 500 mL and T2 (standard temperature) = 0°C + 273 = 273 K

P2 = P1V1T2/T1V2

     = (725 × 375 × 273)/(298 × 500)

     = 498.13 mmHg

1 a

2 d

3 a

4 c

explanation:

oxygen, selenium, tellurium, and polonium.

they're all from the same group as sulfur (group 16).