Question

13. Solid HgO, liquid Hg, and gaseous O2 are placed in a glass bulb and the...

13. Solid HgO, liquid Hg, and gaseous O2 are placed in a glass bulb and the reaction below is allowed to reach equilibrium. 2HgO(s) 2Hg(l) + O2(g); ΔH = +181.6 kJ With the system at equilibrium, the amount of Hg(l) in the bulb can be increasedA) by removing some HgO(s). B) by adding an inert gas. C) by adding some HgO(s). D) by increasing the pressure. E) by increasing the temperature.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The answer is B, I am wondering is the C also correct?? The following reaction is...
The answer is B, I am wondering is the C also correct?? The following reaction is allowed to reach equilibrium is a glass bulb at a given temperature. 2 HgO(s) <---> 2 Hg(l) + O2(g) Delta H = 43.4 kcal/mol. The mass of HgO in the bulb could be increased by: A) removing some Hg B) reducing the volume of the bulb C) adding more Hg D) increasing the temperature E) removing some O
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.
HgO(s) Hg(g) O2(g) Enthaply Delta H kj/mol -90.8 61.3 Entropy Delta S   j/mol. K 70.3 174.9...
HgO(s) Hg(g) O2(g) Enthaply Delta H kj/mol -90.8 61.3 Entropy Delta S   j/mol. K 70.3 174.9 205.0 Above is a table of thermodynamics date for the chemical species in the reaction: 2HgO(s) ----> 2Hg(g)+ O2(g) at 25 C A) Calculate the molar entropy of reaction at 25 C B) Calculate the standard Gibbs free enregy of the reaction at 25 C given that the enthaply of reaction at 25 C is 304.2 Kj/mol C)Calculate the equilibrium constant for the reaction...
1) Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) K=[NO]   / [N2][O2]...
1) Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) K=[NO]   / [N2][O2] K=[NO]2 / [N2][O2] K=[N2][O2]   /   [NO]2 K=2[NO][N2]   /   [O2] 2) The acid HOCl (hypochlorous acid) is produced by bubbling chlorine gas through a suspension of solid mercury(II) oxide particles in liquid water according to the equation 2HgO(s)+H2O(l)+2Cl2(g)⇌2HOCl(aq)+HgO⋅HgCl2(s) What is the equilibrium-constant expression for this reaction? K=[HOCl]2   /   [Cl2]2 K=[HOCl]2[HgO⋅HgCl2]    /   [Cl2]2[H2O][HgO]2 K=[HOCl]2    /     [Cl2]2[H2O] K=[Cl2]2    /    [HOCl]2
How would each of the following changes affect this equilibrium? 2 S(s) + 3 O2(g) ⇌...
How would each of the following changes affect this equilibrium? 2 S(s) + 3 O2(g) ⇌ 2 SO3(g); ΔH = −791.4 kJ/mol (a) increasing the temperature Would it shift the reaction toward the reactants? Would it shift the reaction toward the products? Or, does temp not affect equilibrium? (b) increasing [O2] Does increasing O2 shifts the reaction toward the reactants, shift the reaction toward the products, or does the increasing O2 not affect equilibrium? (c) increasing the volume of the...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are equal b)the value of the equilibrium constant is 1 c)all chemical reactions have ceased d)the rate constants of the forward and reverse reactions are equal e)the limiting reagent has been consumed 2)The equilibrium-constant expression depends on the ________ of the reaction. a) stoichiometry b) mechanism c) the quantities of reactants and products initially present d) temperature e) stoichiometry and mechanism 3)Given the following reaction...
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