A sample of gas occupied 250.0 mL at 30.0 C. What volume will it have at 60.0 C, assuming the pressure remains constant?

274.75 mL

Explanation:

Initial volume of gas V1 = 250.0 mL

Initial temperature of gas T1 = 30.0 C

Convert temperature in Celsius to Kelvin

(30.0°C + 273 = 303K)

New volume V2 = ?

New temperature T2 = 60.0 C

(60.0°C + 273 = 333K)

Since, volume and temperature are involved while pressure is constant, apply the formula for Charles law

V1/T1 = V2/T2

250.0 mL/303K = V2/333K

Cross multiply

250.0 mL x 333K = 303K x V2

83250 = 303V2

V2 = 83250/303

V2 = 274.75 mL

Thus, the volume will be 274.75 mL

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