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| Sections | |||
|---|---|---|---|
| Chemical Equilibrium | 61 mins | 0 completed | Learn Summary |
| ICE Chart | 52 mins | 0 completed | Learn |
| Le Chatelier's Principle | 24 mins | 0 completed | Learn Summary |
| The Reaction Quotient | 11 mins | 0 completed | Learn Summary |
| Additional Practice |
|---|
| Equilibrium Expressions |
Consider the following reaction: H2(g) + I2(g) ⇌ 2HI(g)
Complete the following table. Assume that all concentrations are equilibrium concentrations in M.
| T(oC) | [H2] (M)left[ {{f{H}}_{f{2}} } ight] | [I2] (M) left[ {{f{I}}_{f{2}} } ight] | [HI] (M) left[ {{f{HI}}} ight] | Kcleft[ {{f{K}}_{f{c}} } ight] |
| 25 | 0.0355 | 0.0388 | 0.922 | – |
| 340 | - | 4.60×10−2 | 0.390 | 90.6 |
| 445 | 4.90×10−2 | 4.72×10−2 | – | 50.2 |
Find Kc at 25 oC.
H2(g) + I2(g) ⇌ 2HI(g)
The formula for the equilibrium constant Kc is simply the concentration of the products over the concentration of the reactants with the coefficient of the balanced reaction as the exponent of each concentration term.
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