If an ideal gas has volume V at 27oC and it is heated at constant pressure so that its volume becomes 1.5 V, then the value of final temperature is:

Explanation

Option A: 327 K. This is the temperature if the volume of the gas doubles. However, the volume only increases by 1.5 times, so the temperature will not double. Option B: Initial conditions:Temperature = 27 C = 300 KVolume = VFinal conditions:Volume = 1.5 VTemperature = TCharles's law:V1/T1 = V2/T2 where:V1 is the initial volumeT1 is the initial temperatureV2 is the final volumeT2 is the final temperatureSubstituting the known values into the equation, we get:V/300 = 1.5V/T2 Solving for T2, we get:T2 = 1.5V * 300 / V = 450 K = 177 C Therefore, the final temperature is 177 C.Option C: 873 K. This is the temperature if the volume of the gas triples. However, the volume only increases by 1.5 times, so the temperature will not triple.Option D: 600 C. This is the temperature if the volume of the gas doubles and then increases by 50%. However, the volume only increases by 1.5 times, so the temperature will not increase by 50%.