A sample of gas occupies a volume of 7.50 L at 28.0C. At what temperature is the volume of the gas 4.00 L if the pressure is kept constant.

Explanation:

To solve this, you must use Charles' Law:

V1/T1 = V2/T2

The values given are:

V1 = 7.50 L

V2 = 4.00 L

Temperature must be in Kelvin

Conversion: 28+273 = 301 K

Substitute values in Charles' Law:

7.50L /301 K = 4.00/T2

Cross-Multiply:

(7.50)(T2) = 1204

Solve for T2:

T2 = 160.53 K or -112.47˚C

This makes sense, as volume and temperature are directly proportional. As V increases, so will T and vice versa.

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.

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i