A 251-mL sample of a gas at STP is heated to 45°C. The final pressure is 1.10 atm. Calculate the volume of this gas under the new conditions.

The volume of the gas under the new conditions is 266 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. We convert the unit Celsius into Kelvin:

0 ° C = 273K, 45 ° C = 273 + 45 = 318K. The conditions STP are: 1 stm of pressure and 273K of temperature.

P1xV1/T1= P2xV2/T2

1 atmx 251ml/273K=1,10atmx V2/318K

0,92 atmx L/K = 1,10atmx V2/318K

V2= (0,92 atmx L/K x 318K)/1,10 atm= 265, 79 ml

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

it would be a gas formation