It would be to change the amount of solute or solvent in the solution.
Answer:
photosynthesis
Explanation:
its the first step of the cycle
Answer:
burning of wood is an irreversible change bcoz wood after burning wood converted to ashes cannot be converted back to wood nd its chemical composition also changes
Answer:
![[H_2]_{eq}=0.183M](https://tex.z-dn.net/?f=%5BH_2%5D_%7Beq%7D%3D0.183M)
![[I_2]_{eq}=0.183M](https://tex.z-dn.net/?f=%5BI_2%5D_%7Beq%7D%3D0.183M)
![[HI]_{eq}=0.025M](https://tex.z-dn.net/?f=%5BHI%5D_%7Beq%7D%3D0.025M)
Explanation:
Hello.
In this case, for this equilibrium problem, we first realize that at the beginning there is just HI, it means that the reaction should be rewritten as follows:

Whereas the law of mass action (equilibrium expression) is:
![Kc=\frac{[H_2][I_2]}{[HI]^2}](https://tex.z-dn.net/?f=Kc%3D%5Cfrac%7B%5BH_2%5D%5BI_2%5D%7D%7B%5BHI%5D%5E2%7D)
That in terms of initial concentrations and reaction extent or change
turns out:
![Kc=\frac{x*x}{([HI]_0-2x)^2}\\\\54.3=\frac{x^2}{(0.391M-2x)^2}](https://tex.z-dn.net/?f=Kc%3D%5Cfrac%7Bx%2Ax%7D%7B%28%5BHI%5D_0-2x%29%5E2%7D%5C%5C%5C%5C54.3%3D%5Cfrac%7Bx%5E2%7D%7B%280.391M-2x%29%5E2%7D)
And the solution via solver or quadratic equation is:

Whereas the correct answer is 0.183 M since the other value yield a negative concentration of HI at equilibrium (0.391-2*0.210=-0.029M).This, the equilibrium concentrations are:
![[H_2]_{eq}=0.183M](https://tex.z-dn.net/?f=%5BH_2%5D_%7Beq%7D%3D0.183M)
![[I_2]_{eq}=0.183M](https://tex.z-dn.net/?f=%5BI_2%5D_%7Beq%7D%3D0.183M)
![[HI]_{eq}=0.391M-2*0.183M=0.025M](https://tex.z-dn.net/?f=%5BHI%5D_%7Beq%7D%3D0.391M-2%2A0.183M%3D0.025M)
Regards.
Answer:
The Kc of this reaction is 311.97
Explanation:
Step 1: Data given
Kp = 0.174
Temperature = 243 °C
Step 2: The balanced equation
N2(g) + 3H2(g) ⇌ 2NH3(g)
Step 3: Calculate Kc
Kp = Kc *(RT)^Δn
⇒ with Kp = 0.174
⇒ with Kc = TO BE DETERMINED
⇒ with R = the gas constant = 0.08206 Latm/Kmol
⇒ with T = the temperature = 243 °C = 516 K
⇒ with Δn = number of moles products - moles reactants 2 – (1 + 3) = -2
0.174 = Kc (0.08206*516)^-2
Kc = 311.97
The Kc of this reaction is 311.97