Question

I need help with this for practice, I have a test Friday. Thank you in advance!

1. Consider the equilibrium system involving the decomposition of nitrogen monoxide.

2NO(g) <>N2(g) + O2(g)

K = [N2] [O2] = 2.78×10-2 at 287 K   [NO]2

A flask originally contains 0.226 M nitrogen monoxide. Calculate the equilibrium concentrations of the three gases.

[NO]	=	M
[N2]	=	M
[O2]	=	M

2. A student ran the following reaction in the laboratory at 278 K:

2CH₂Cl₂(g)<> CH₄(g) + CCl₄(g)  

When she introduced 7.77×10^-2 moles of CH₂Cl₂(g) into a 1.00 liter container, she found the equilibrium concentration of CH₂Cl₂(g) to be 4.87×10^-3 M.  

Calculate the equilibrium constant, K_c, she obtained for this reaction.

3. The equilibrium constant, K_c, for the following reaction is 1.80×10^-4 at 298 K.

NH₄HS(s) <>NH₃(g) + H₂S(g)  

Calculate the equilibrium concentration of H₂S when 0.546 moles of NH₄HS(s) are introduced into a 1.00 L vessel at 298 K.  

Answer 1

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