Chemeq_part1 Additional Exercises

I.

Write expressions for KC, and KP if applicable for the following reversible reactions. 1. Sb2S3(s) + H2(g)  Sb(s) + H2S(g) 2. Fe3O4(s) + H2(g)  FeO(s) + H2O(g) 3. CN-(aq) + H2O (l)  HCN(aq) + OH-(aq)

II.

1. 2. 3. 4. 5. III.

The initial condition of pressure or concentration is given below the formula of each species in each of the following equations. Evaluate QC or QP for each reaction, compare the value with the given KC or KP. Based on this, predict if the reaction will shift forward, backward or if it is at equilibrium. CH4(g) + CCl4(g)  2CH2Cl2(g) KC = 0.0956 at 298 K 0.207 M 0.0156 M 0.0142 M N2(g) + 3H2(g)  2NH3(g) KC = 1.4 x 105 at 473 K 0.214 M 0.0163 M 0.270 M PCl3(g) + Cl2(g)  PCl5(g) KC = 1.784 AT 600 K 0.149 M 0.0172 M 0.206 M H2(g) + CO2(g)  H2O(g) + CO(g) KP = 8.31 x 10-3 at 500 K 0.300 atm 0.406 atm 0.0411 atm 0.114 atm PCl5(g)  PCl3(g) + Cl2(g) KP = 0.675 at 500 K 0.543 atm 0.121 atm 0.121 atm

Use the following data at 1200 K to estimate the value of KP for the reaction 2H2(g) + O2(g)  2H2O(g) C(graphite) + CO2(g)  2CO(g) KC = 0.64 CO2(g) + H2(g)  CO(g) + H2O(g) KC = 1.4 C(graphite) + ½ O2(g)  CO(g) KC = 1.0 x 108

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