For the reaction H2(g) + I2(g) ↔ 2 HI(g), you have the initial concentrations [H2] = 0.15 and [I2] = 0.05. Keq for the reaction at this temperature is 4.5 x 10-6. Make a reaction table. Include rows for initial concentration, change in concentration, and equilibrium concentration. Write down the equation for Keq. Solve for x. What are the equilibrium concentrations for H2, I2, and HI?

Question

For the reaction H2(g) + I2(g) ↔ 2 HI(g), you have the initial concentrations [H2] = 0.15 and [I2] = 0.05. Keq for the reaction at this temperature is 4.5 x 10-6. Make a reaction table. Include rows for initial concentration, change in concentration, and equilibrium concentration. Write down the equation for Keq. Solve for x. What are the equilibrium concentrations for H2, I2, and HI?

Answer 1

some hydrogen and iodine are mixed

Answer 2

To create a reaction table, we first write down the balanced chemical equation for the reaction:

H2(g) + I2(g) ↔ 2 HI(g)

Next, we create a table with the columns labeled "Initial Concentration," "Change in Concentration," and "Equilibrium Concentration." We also include rows for each of the reactants and products:

Reactants:
H2(g) | | |
I2(g) | | |

Products:
HI(g) | | |

Next, we fill in the initial concentrations given in the question:

Reactants:
H2(g) | 0.15 | |
I2(g) | 0.05 | |

Products:
HI(g) | | |

Since we are not given the values for the equilibrium concentrations, we leave those cells blank for now.

To find the change in concentration, we need to determine the stoichiometric coefficients of each substance.

From the balanced equation, we see that the stoichiometric coefficient for H2 is 1, for I2 is 1, and for HI is 2.

Next, we can express the change in concentration in terms of x, which represents the change in concentration for any of the substances.

Reactants:
H2(g) | 0.15 | -x |
I2(g) | 0.05 | -x |

Products:
HI(g) | 2x | |

Now, let's calculate the equilibrium concentrations by subtracting x from the initial concentrations for H2 and I2, and adding 2x to find the equilibrium concentration of HI:

Reactants:
H2(g) | 0.15 - x | -x |
I2(g) | 0.05 - x | -x |

Products:
HI(g) | 2x | |

Now, we can write the equation for the equilibrium constant, Keq:

Keq = [HI]^2 / ([H2] * [I2])

Given that Keq for the reaction at this temperature is 4.5 x 10^(-6), we can substitute the equilibrium concentrations into the equation and solve for x.

4.5 x 10^(-6) = (2x)^2 / ((0.15 - x) * (0.05 - x))

Solving this equation for x will give us the value of x, which represents the change in concentration at equilibrium.

Once we have the value of x, we can substitute it back into the equilibrium concentrations equation to find the equilibrium concentrations for H2, I2, and HI.