Question

At what temperature (in

c.does 121 ml of co2 at 27c and 1.05 atm occupy a volume of 293 ml at a pressure of 1.40 atm?

Answer 1

Answer: The final temperature is coming out to be 704.9°C

Step-by-step explanation:

To calculate the temperature when pressure and volume has changed, we use the equation given by combined gas law. The equation follows:

`(P_1V_1)/(T_1)=(P_2V_2)/(T_2)`

where,

`P_1,V_1\text{ and }T_1` are the initial pressure, volume and temperature of the gas

`P_2,V_2\text{ and }T_2` are the final pressure, volume and temperature of the gas

We are given:

`P_1=1.05atm\\V_1=121mL\\T_1=27^oC=[27+273]K=300K\\P_2=1.40atm\\V_2=293mL\\T_2=?K`

Putting values in above equation, we get:

`(1.04atm* 121mL)/(300K)=(1.40atm* 293mL)/(T_2)\\\\T_2=(1.40* 293* 300)/(1.04* 121)=977.9K`

Converting the temperature from kelvins to degree Celsius, by using the conversion factor:

`T(K)=T(^oC)+273`

`977.9=T(^oC)+273\\T(^oC)=704.9^oC`

Hence, the final temperature is coming out to be 704.9°C

Answer 2

For the above question we can use the combined gas law,

`(P1V1)/(T1) = (P2V2)/(T2)`
where P - pressure, T- temperature and V- volume
temperature has been given in celsius, we have to convert into Kelvin scale to calculate.
temperature in Kelvin = temperature in celcius + 273
27 °C + 273 = 300 K

`(1.05 atm*121 mL)/(300K) = (1.40 atm*293 mL )/(T)`
T = 967 K
Temperature in celcius - 969 - 273 = 696 °C