Gas initially at a temperature of 17°Cand pressure 150 kPa is heated at constant volume until its temperature is 124°C. Determine the final pressure of the gas, assuming no loss of gas.a.20.35 kPAb.203.5 kPAc.203.5 Pad.2.035 kPaClear my choice

To solve this problem, we can use the ideal gas law, which states that the pressure of a gas is directly proportional to its temperature, if the volume and the amount of gas are kept constant. This relationship can be expressed as P1/T1 = P2/T2, where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.

Step 1: Convert all temperatures to Kelvin. The Kelvin scale is the standard unit of temperature in physics, and it starts at absolute zero, the point at which all molecular motion ceases. To convert from Celsius to Kelvin, add 273.15.

T1 = 17°C + 273.15 = 290.15 K T2 = 124°C + 273.15 = 397.15 K

Step 2: Substitute the known values into the equation and solve for P2.

P1/T1 = P2/T2 150 kPa / 290.15 K = P2 / 397.15 K P2 = (150 kPa * 397.15 K) / 290.15 K P2 = 205.3 kPa

So, the final pressure of the gas, assuming no loss of gas, is approximately 205.3 kPa. The closest answer to this is 203.5 kPa (option b).