What are the final concentrations of A and A2 at equilibrium if the initial [A2] concentration is 0.60M?
A2 (g) ⇌ 2A(g)
K = 4.2 x 10-8
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I2. I− Initial. 2mol/2L = 1 M. Change. −x. +2x. Equilibrium. 1−x. 2x. At equilibrium. ...
1 . Ag+ Cl− Initial. 0.02mol/1.00 L = 0.02 M. Change.
2 . +x. +x. Equilibrium. x. 0.02+x. Kc=[Ag−][Cl−] ...
3 . H2CO3. SO2−4. H3O+ Initial. 0.4. 0.01. 0.07. Change. −x. +x. ...
4 . H2CO3 H+ CO2−3. Initial. .16. Change. -x. +x. +x. Equilibrium. ...
5 . First write out the balanced equation:
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