At 35oC, K = 1.6 10-5 for the reaction 2NOCl(g) 2NO(g) + Cl2(g) Calculate the
Question:
2NOCl(g) ⇌ 2NO(g) + Cl2(g)
Calculate the concentrations of all species at equilibrium for each of the following original mixtures.
a. 2.0 moles of pure NOCl in a 2.0- L flask
b. 2.0 moles of NO and 1.0 mole of Cl2 in a 1.0- L flask
c. 1.0 mole of NOCl and 1.0 mole of NO in a 1.0- L flask
d. 3.0 moles of NO and 1.0 mole of Cl2 in a 1.0- L flask
e. 2.0 moles of NOCl, 2.0 moles of NO, and 1.0 mole of Cl2 in a 1.0- L flask
f. 1.00 mol/ L concentration of all three gases
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Step by Step Answer:
a The reaction must proceed to products to reach equilibrium because only reactants are present initially Summarizing the problem in a table 2 NOClg 2 NOg Cl 2 g K 16 10 5 Initial 10 M 0 0 2 x molL of ...View the full answer
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