At a pressure of 780.0 mmHg and 25.2 C, a certain gas has a volume of 350.0 mL. What will be the volume of this gas under STP

The volume will be 0,330 L (330 ml).

Explanation:

We use the gas formula, which results from the combination of the Boyle, Charles and Gay-Lussac laws. According to which at a constant mass, temperature, pressure and volume vary, keeping constant PV / T. The conditions STP are 1 atm of pressure and 273 K of temperature. We convert the unit Celsius into Kelvin, the volume in ml into L and the pressure in mmHg into atm:

0 ° C = 273K, 25,2= 273 + 25, 2= 298,2K ;  350/1000= 0,350 L

760 mmHg1 atm

780 mmHgx= (780 mmHgx 1 atm)/760 mmHg=1, 03 atm

P1xV1/T1= P2xV2/T2

V2 =((P1xV1/T1)xT2)/P2

V2=((1, 03 atmx 0,350 L/298,2K)x273K)/1 atm= 0,330 L

why do the isotopes of a particular element behave differently in nuclear reactions but the same in chemical reactions? chemical reactions involve changes to electrons in an atom; isotopes do not differ in electrons, and so they react the same way during chemical changes.

i think its 100.

hope this !