Question

Suppose a 250. mL flask is filled with 1.8 mol of CO, 1.5 mol of H2) and 1.9 mol of CO2. The following reaction becomes possible: CO (g) + H2O (g) = CO2 (g) + H2 (g). The equilibrium constant K for this reaction is 0.724 at the temperature of the flask. Calculate the equilibrium molarity of H2O.

Name: suppose a 250 ml flask is filled with 18 mol of co 15 mol of h2 and 19 mol of co2 the following reaction becomes possible co g h2o g co2 g h2 g the equilibrium constant k for this reaction i 16033
Uploaded: 2023-03-27T05:11:29-08:00
Duration: 3 min 24 s
Channel: Ronald Prasad
Description: suppose a 250 ml flask is filled with 18 mol of co 15 mol of h2 and 19 mol of co2 the following reaction becomes possible co g h2o g co2 g h2 g the equilibrium constant k for this reaction i 16033

          Suppose a 250. mL flask is filled with 1.8 mol of CO, 1.5 mol of H2) and 1.9 mol of CO2. The following reaction becomes possible: CO (g) + H2O (g) = CO2 (g) + H2 (g). The equilibrium constant K for this reaction is 0.724 at the temperature of the flask. Calculate the equilibrium molarity of H2O.

Added by Alicia C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ronald Prasad

03/27/2023

Step 1

- Volume of the flask = 250 mL = 0.250 L - Initial moles of CO = 1.8 mol - Initial moles of H2O = 1.5 mol - Initial moles of CO2 = 1.9 mol Initial concentrations: - [CO] = moles/volume = 1.8 mol / 0.250 L = 7.2 M - [H2O] = 1.5 mol / 0.250 L = 6.0 M - [CO2] = 1.9 Show more…

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Suppose a 250. mL flask is filled with 1.8 mol of CO, 1.5 mol of H2) and 1.9 mol of CO2. The following reaction becomes possible: CO (g) + H2O (g) = CO2 (g) + H2 (g). The equilibrium constant K for this reaction is 0.724 at the temperature of the flask. Calculate the equilibrium molarity of H2O.