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.

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

i believe the answer is true.