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Chemistry, 19.09.2019 20:30 lulabelles7750
Given the following balanced equation at 120°c: a(g) + b(g) ⇋ 2 c(g) + d(s)(a) at equilibrium a 4.0 liter container was found to contain 1.60 moles of a, and 0.40 moles of b, and 0.40 moles of c, and 1.60 moles of d. calculate kc.(b) if 0.20 moles of b and 0.20 mole of c are added to this system, what will be the new equilibrium concentration of a be? (c) if the volume of the container in which the system is at equilibrium [part (a)] is suddenly halved, what will be the new equilibrium concentrations?
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Given the following balanced equation at 120°c: a(g) + b(g) ⇋ 2 c(g) + d(s)(a) at equilibrium a 4.0...
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