Question

Medal and fan
The equilibrium constant for the formation of phosphorus pentachloride is 1.9. If the partial pressure of each gas is .5 atm, will the reaction proceed forward or backward to reach equilibrium?
PCl3 (g) + Cl2 <-> PCl5 (g)

A. Backward, because K is less than Q.
B. Backward because K is greater the Q.
C. Forward, because K is greater than Q
D. Forward, because K is less than Q.

The partial pressures of the gas confuse me.

Thanks(:

The partial pressures in the equation confuse me.

Answer 1

@Abhisar

Answer 2

@Somy

Answer 3

@aaronq

Answer 4

@JFraser

Answer 5

Find Q with what you're given and compare it to K

Answer 6

How do you find Q with partial pressures?

Answer 7

partil pressures are analogous to concentrations

Answer 8

u know how to work with Kc right?

Answer 9

its same with Kp

Answer 10

plug the pressures into an equation that looks just like K, but it will tell you whether or not the concentrations are right to be at equilibrium

Answer 11

Kp= product/reactant

Answer 12

Well, then Q would be less than K, correct?

Answer 13

looks like that
let me check with Pa unit

Answer 14

gas pressures can be used in equilibrium just like concentrations, and get plugged into a Q equation the exact same way

Answer 15

oh im getting a crazy number

Answer 16

I'm being dumb, Q is more than K, I had the reactants and products mixed up. That would mean the reaction is reversed.

Answer 17

i guess so
im not as good in this and u already know :D

Answer 18

Haha neither am I. This section is the only section that has given me problems so far.