post assessment questions

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post assessment questions

Postby josephyim1L » Wed Jan 09, 2019 5:17 pm

Can someone explain this question to me:

15. Carbonyl chloride (COCl2 ), also called phosgene, was used in World War I as a poisonous gas. The equilibrium concentrations for the reaction between carbon monoxide and molecular chlorine to form carbonyl chloride at 74℃ are [CO] = 1.2 x 10-2 M, [Cl2 ] = 0.054 M, and [COCl2 ] = 0.14 M. Calculate the equilibrium constant for this reaction: CO (g) + Cl2 (g) ⇌ COCl2 (g)

I'm not sure how to utilize PV=nRT to find the solution to this question.

Nada AbouHaiba 1I
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Re: post assessment questions

Postby Nada AbouHaiba 1I » Wed Jan 09, 2019 5:20 pm

To find the equilibrium constant you'll just use the equation concentration of the products/concentrations of the reactants, not pv=nrt.

Ashley Zhu 1A
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Joined: Fri Sep 28, 2018 12:16 am

Re: post assessment questions

Postby Ashley Zhu 1A » Wed Jan 09, 2019 5:51 pm

since the given chemical equation is all gases, you can rearrange the pv = nrt equation to p = nrt/v = Mrt (where M is molarity for concentration since n/V is mol/L) to find the partial pressures of the gases from the given concentrations; then, you can find the equilibrium constant using P(products)/P(reactants)

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