Question

Suppose a 500. mL flask is filled with 0.60 mol of H2 and 0.20 mol of I2. The following reaction becomes possible: H2(g) + I2(g) ? 2HI(g) The equilibrium constant K for this reaction is 3.18 at the temperature of the flask. Calculate the equilibrium molarity of I2. Round your answer to two decimal places.

          Suppose a 500. mL flask is filled with 0.60 mol of H2 and 0.20 mol of I2. The following reaction becomes possible:
H2(g) + I2(g) ? 2HI(g)
The equilibrium constant K for this reaction is 3.18 at the temperature of the flask.
Calculate the equilibrium molarity of I2. Round your answer to two decimal places.

Suppose a 500. mL flask is filled with 0.60 mol of H2 and 0.20 mol of I2. The following reaction becomes possible:
H2(g) + I2(g) ? 2HI(g)
The equilibrium constant K for this reaction is 3.18 at the temperature of the flask.
Calculate the equilibrium molarity of I2. Round your answer to two decimal places.

Added by Kevin C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

07/24/2023

Step 1

First, we need to find the initial molarity of Hz and Iz. Molarity = moles/volume Molarity of Hz = 0.60 mol / 0.500 L = 1.20 M Molarity of Iz = 0.20 mol / 0.500 L = 0.40 M Show more…

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Suppose a 500 mL flask is filled with 0.60 mol of H2 and 0.20 mol of I2. The following reaction becomes possible: H2(g) + I2(g) ℌ 2HI(g) The equilibrium constant K for this reaction is 3.18 at the temperature of the flask. Calculate the equilibrium molarity of I2. Round your answer to two decimal places.