A sealed container was filled with 0.5 moles of H2(g), 0.7 moles of I2(g) and 0.1 moles of HI(g) at 945 K. The initial total pressure in the container was 1 bar. Calculate the amounts of each components in the mixture at equilibrium for the reaction H2(g)+I2(g) *) 2 HI(g). You may not assume that the entropies and enthalpies are temperature independent.

answers

watching

views

For unlimited access to Homework Help, a Homework+ subscription is required.

Join us on Discord

Chemistry Study Group

Join now

Related questions

The equilibrium constant, K_p, for the following reaction is 10.5 at 350K.

2CH₂Cl₂(g) ----->CH₄(g) + CCl₄(g)

If an equilibrium mixture of the three gases in a 13.3 L container at 350K contains CH₂Cl₂ at a pressure of 0.309 atm and CH₄ at a pressure of 0.289 atm, the equilibrium partial pressure of CCl₄ is atm.

2. Consider the following reaction:

2HI(g) ---->H₂(g) + I₂(g)

If 2.41 moles of HI, 0.363 moles of H₂, and 0.398 moles of I₂ are at equilibrium in a 12.9 L container at 853 K, the value of the equilibrium constant, K_p, is .

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature, 0.7 mol of H2 and 0.7 mol of I2 were placed in a 1 L container. What is the concentration of HI present at equilibrium?

H₂(g) + I₂(g) <-> 2HI(g)

K_p= 0.456 at 398K

Assume that initially there are n moles of HI in a varaible volume priston and no moles of H₂ and I₂ are present.

a) Find the partial pressures of HI, HI₂, and I₂ when the piston is set to give 1.00 bar total pressure.

b) Find Î_rG^o

Weekly leaderboard

Home

Homework Help 3,900,000

Chemistry 830,000

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

Related questions

Weekly leaderboard