A sample of oxygen gas at a pressure of 1.14 atm and a temperature of 21.5 degrees Celsius, occupies a volume of 815 ml. If the gas is compressed at constant temperature until it’s pressure is 1.62 atm, the volume of the gas will be what?

The volume of the gas will be 573.52 mL.

Explanation:

Boyle’s law states that the  pressure of a fixed amount of gas at a constant temperature is inversely proportional  to the volume of the gas.

The equation for Boyle's law is:

P₁V₁ = P₂V₂

We want to know V₂, that is, the volume of the container after the compression. We rearrange the equation and calculate:

V₂ = P₁V₁ ÷ P₂

V₂ = 1.14 atm × 815 mL ÷ 1.62 atm = 573.52 mL

answer is: c. the experiment shows that the red substance experienced a chemical change.

this is chemical change (chemical reaction), because two new substances are formed (metalig liquid and gas), the atoms are rearranged and the reaction is followed by an energy change.

this is example of chemical decomposition.

chemical decomposition (analysis) is the separation of a single chemical compound into its two or more elemental parts or to simpler compounds.  

chemical decomposition is opposite of chemical synthesis.

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