Question

A gas has an initial volume of 17.2 Liters, a temperature of -15 Celsius, and a

pressure of 1.45 atm. If the temperature is increased to 39 Celsius, and the
volume increases to 164 Liters, what would the final pressure of this gas be?

Answer 1

Using the combined gas law, which is P1V1/T1 = P2V2/T2, we can calculate the final pressure of the gas after temperature and volume changes. We first convert temperatures to Kelvin, then substitute the known values into the equation and solve for P2 to get the final pressure in atmospheres.

Step-by-step explanation:

To find the final pressure of the gas given the changes in volume and temperature, we can use the combined gas law which is P1V1/T1 = P2V2/T2. Given that V1 is 17.2 Liters, T1 is -15 Celsius (which we need to convert to Kelvin by adding 273 to get 258 K), P1 is 1.45 atm, V2 is 164 Liters, and T2 is 39 Celsius (which needs to be converted to Kelvin by adding 273 to get 312 K). We can solve for P2 by rearranging the combined gas law to P1V1/T1 = P2V2/T2 becomes P2 = P1V1T2/(T1V2). Substituting in the known values and solving for the final pressure gives us:

P2 = (1.45 atm * 17.2 L * 312 K) / (258 K * 164 L)

After the calculations, we would get the final pressure P2 in atmospheres.