a sample of gas at a pressure of 5.1 atm and a temperature of 45 degrees celsius is heated. it's pressure goes to 7.8 atm what is it's new temperature in celsius

213.4°C.

Explanation:

Data obtained from the question:

Initial pressure (P1) = 5.1atm

Initial temperature (T1) = 45°C = 45°C + 273 = 318K

Final pressure (P2) = 7.8atm

Final temperature (T2) = ... ?

The new temperature can be obtained as follow:

P1/T1 = P2 / T2

5.1/318 = 7.8/T2

Cross multiply

5.1 x T2 = 318 x 7. 8

Divide both side by 5.1

T2 = 318 x 7. 8 / 5.1

T2 = 486.4K

Finally, we shall convert 486.4K to celsius temperature. This can be done as follow:

T (°C) = T (K) - 273

T (K) = 486.4K

T (°C) = 486.4 - 273

T (°C) = 213.4°C.

Therefore, the new temperature is 213.4°C