Question

Liquid mercury can be generated by heating solid mercury (II) oxide to decomposition, releasing oxygen gas....

Liquid mercury can be generated by heating solid mercury (II) oxide to decomposition, releasing oxygen gas. 2HgO(s) 2Hg(l) + O2(g) If you place a specific amount of the solid mercury compound in a closed reaction vessel at a particular temperature and allow equilibrium to be reached, how could you then increase the formation elemental mercury? (select all that apply)

Adding more mercury(II) oxide.

Removing some oxygen.

Increasing the volume of the vessel.

Homework Answers

Answer #1

By Removing some oxygen and increasing the volume of the vessel we can increase the formation of elemental mercury.

Explanation: Adding more mercury (II) oxide will not show any effect on equilibrium as solids do not have any effect on equilibrium.

removing oxygen will shift the equilibrium towards right side in order to increase the decreased amount of oxygen.

Increasing volume will decrease the pressure which will shift the equilibrium in that direction where the number of moles of gaseous reactants are high that is towards right side.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
To the correct number of significant figures a 323 gram solid cube of mercury (II) oxide...
To the correct number of significant figures a 323 gram solid cube of mercury (II) oxide has a density of 4.2 x 104 ng/m3 . a) What is the length of one side of the cube in cm? b) The mercury (II) oxide completely dissociates and forms liquid mercury and oxygen gas. Write a balanced chemical equation and indicate if this process is a chemical or physical change? c) The oxygen gas escapes and now you are left with liquid...
Joseph Priestly prepared oxygen in 1774 by heating red mercury(II) oxide with sunlight focused through a...
Joseph Priestly prepared oxygen in 1774 by heating red mercury(II) oxide with sunlight focused through a lens. How much heat (in kJ) is required to decompose 1.42 mol of red HgO(s) to Hg(l) and O2(g) under standard conditions? (Hint: Use the Supporting Material.) ______kJ
The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury (II) oxide. HgO(s)...
The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury (II) oxide. HgO(s) --> Hg(l) + 1/2O2(g) ΔH° = 90.84 kJ Use the data given below to determine DS =    and the temperature, at which this reaction will become spontaneous under standard conditions. S°(Hg) = 76.02 J/K· mol S°(O2) = 205.0 J/K· mol S°(HgO) = 70.29 J/K· mol
Procedure Reaction 1: Dissolving the Copper 1. Obtain a clean, dry, glass centrifuge tube. 2. Place...
Procedure Reaction 1: Dissolving the Copper 1. Obtain a clean, dry, glass centrifuge tube. 2. Place a piece of copper wire in a weighing paper, determine the mass of the wire and place it in the centrifuge tube. The copper wire should weigh less than 0.0200 grams. 3. In a fume hood, add seven drops of concentrated nitric acid to the reaction tube so that the copper metal dissolves completely. Describe your observations in the lab report. (Caution, Concentrated nitric...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT