Question

7. A 26.4-ml sample of ethylene gas, C2H4, has a pres-sure of 2.50 atm at 2.5°C. If the

volume is increased to 36.2 mL and the temperature is raised to 10°C, what is the
new pressure. (Hint: Three variables have been given so what equation will you
use?)

Answer 1

Answer: 1.87 atm

Step-by-step explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

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

where,

`P_1` = initial pressure of gas = 2.50 atm

`P_2` = final pressure of gas = ?

`V_1` = initial volume of gas = 26.4 ml

`V_2` = final volume of gas = 36.2 ml

`T_1` = initial temperature of gas =
`2.5^oC=273+2.5=275.5K`

`T_2` = final temperature of gas =
`10^oC=273+10=283K`

Now put all the given values in the above equation, we get:

`(2.50* 26.4)/(275.5)=(P_2* 36.2)/(283)`

`P_2=1.87atm`

The new pressure is 1.87 atm by using combined gas law.