Question

A reaction requires 1.5 mL of ammonia if it occurs at 1.65 atm and 23 degrees celsius. If the temperature is changed to 30 degrees celsius, what will the new pressure be if the volume remains the same?

Answer 1

Answer: The new pressure will be 1.69 atm

Step-by-step explanation:

Gay-Lussac's law states that the pressure of the gas is directly proportional to the temperature of the gas at constant volume and the number of moles.

Mathematically,

`P\propto T` (At constant volume and number of moles)

OR

`(P_1)/(T_1)=(P_2)/(T_2)` .....(1)

`P_1\text{ and }T_1` are the pressure and temperature of the gas

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

We are given:

`P_1=1.65atm\\T_1=23^oC=[23+273]K=296K\\V_2=?mL\\T_2=30^oC=[30+273]K=303K`

Putting values in equation 1, we get:

`(1.65atm)/(296K)=(P_2)/(303K)\\\\P_2=(1.65* 303)/(296)\\\\P_2=1.69atm`

Hence, the new pressure will be 1.69 atm