Question

Multiple Choice/short answer Practice for Equilibrium Write a short explanation for your choice of answer, although...

Multiple Choice/short answer Practice for Equilibrium

Write a short explanation for your choice of answer, although the explanation will not be graded neither will your answer be graded without one! Questions with a star (*) may have more than one correct answer. Report all correct answers.

Questions below refer to the following exothermic reaction

H2(g) + Cl2(g) + C(s) → CH2Cl2(g)   

KP = 0.048

rate = (4.0 x 103s-1)[H2]

____________ 1. This reaction will
a. make a lot of product quickly

b. make very little product quickly

c. make a lot of product slowly

d. make very little product slowly

____________ 2. The KC value will be

a. 0.048

b. greater than 0.048

c. less than 0.048

3. What is the value of Kp for CH2Cl2(g) → H2(g) + Cl2(g) + C(s)

_____________ 4. If more carbon were added to the system at equilibrium, the concentration of hydrogen would
a. increase

b. decrease

c. stay the same

d. more information is needed to predict

_____________ 5. If chlorine was removed from the system at equilibrium, the concentration of hydrogen would

a. increase

b. decrease

c. stay the same

d. more information is needed to predict

______________ 6. If the reaction were conducted at a higher temperature, the concentration of hydrogen would

a. increase

b. decrease

c. stay the same

d. more information is needed to predict

7. If the reaction were conducted at a smaller volume, the concentration of hydrogen would

a. increase

b. decrease

c. stay the same

d. more information is needed to predict

8*. Changing which of the following will change the value of the equilibrium constant?

a. adding carbon
d. changing volume

b. removing chlorine

e. adding a catalyst

c. increasing temperature

__________ 9. The value of ΔG ̊ will be
a. positive

b. negative

c. greater than 1

d. less than 1

__________ 10. If 1.0 mol of each reactant and product were added to a 1.0 L flask, at equilibrium the concentration of dichloromethane will be

a. 1.0 M

b. greater than 1.0 M

c. less than 1.0 M

I would please like to know the explanations to all of the answers. Note that #8 has more than one right answer.

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
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...
5) (10 pts) For the endothermic reaction below initially at equilibrium, predict the shift in the...
5) (10 pts) For the endothermic reaction below initially at equilibrium, predict the shift in the reaction for each of the following scenarios. C(s) + H2O (g) ⇌ CO (g) + H2 (g) Disturbance Shift (left/right) a. Increase the amount of Water b. Decrease the pressure by half c. Remove C from the reaction d. Add hydrogen to the mixture e. Increase the temperature
CO2 and H2 are allowed to react until equilibrium is established as follows: CO2(g) + H2(g)...
CO2 and H2 are allowed to react until equilibrium is established as follows: CO2(g) + H2(g) ↔ H2O(g) + CO(g) Which of the following changes will cause the equilibrium position to shift to the right? a. increase in the concentration of H2 b. decrease in the concentration of CO c. decrease in the concentration of CO2 d. more than one correct response e. no correct response
Calculating Equilibrium Constants. The equilibrium constant, K, of a reaction at a particular temperature is determined...
Calculating Equilibrium Constants. The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium. For a gaseous reaction with the general form aA+bB⇌cC+dD the Kc and Kp expressions are given by Kc=[C]c[D]d[A]a[B]b Kp=(PC)c(PD)d(PA)a(PB)b The subscript c or p indicates whether K is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved...
Indicate how each of the following will affect the equilibrium concentration of NH3 in the following...
Indicate how each of the following will affect the equilibrium concentration of NH3 in the following reaction: 4NH3(g)+5O2(g)?4NO(g)+6H2O(g)+906kJ Part A adding more O2(g) a. The equilibrium concentration of NH3 will decrease. b. The equilibrium concentration of NH3 will increase. c. The equilibrium concentration of NH3 will not change. Part B increasing the temperature of the reaction a. The equilibrium concentration of NH3 will increase. b. The equilibrium concentration of NH3 will decrease. c. The equilibrium concentration of NH3 will not...
Consider the reaction: N2(g) + 3H2(g) → 2NH3(g). At a particular moment during the reaction hydrogen...
Consider the reaction: N2(g) + 3H2(g) → 2NH3(g). At a particular moment during the reaction hydrogen is being consumed at a rate of 0.074 M/s. At this moment: (a) What is the rate of reaction (in M/s)? {3 points} (b) A what rate (in M/s) is NH3 being produced? {3 points} (c) Are these average or instantaneous rates? {1 point} [3] A certain first-order reaction has a rate constant of 1.65 min-1 at 20°C. What is the value of the...
The reaction below has an equilibrium constant of Kp=2.26×104 at 298 K. CO(g)+2H2(g)⇌CH3OH(g) Part A Calculate...
The reaction below has an equilibrium constant of Kp=2.26×104 at 298 K. CO(g)+2H2(g)⇌CH3OH(g) Part A Calculate Kp for the reaction below. CH3OH(g)⇌CO(g)+2H2(g) K = Part B Predict whether reactants or products will be favored at equilibrium in the reaction above. Products will be favored at equilibrium. Reactants will be favored at equilibrium. Part C Calculate Kp for the reaction below. 12CO(g)+H2(g)⇌12CH3OH(g) K = Part D Predict whether reactants or products will be favored at equilibrium in the reaction above. Products...
Refer to the reaction system C(s) + H2O(g) ↔ CO(g) + H2(g) at equilibrium for which...
Refer to the reaction system C(s) + H2O(g) ↔ CO(g) + H2(g) at equilibrium for which ΔH°rxn = +131 kJ. Assume ideal gas behavior. Predict the direction in which the above equilibrium will shift as a result of the stated change in conditions. a) An increase in the reaction temperature. b) A decrease in the amount of C(s). c) A decrease in the reactor volume. d) An increase in PH2O. e) Addition of N2 gas to the reaction mixture.
The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g)...
The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) If 0.35 moles of CO2 and 0.35 moles of H2 are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached? The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) If 0.35 moles of CO2 and 0.35 moles of...
1. For the reaction: 2NOCl(g) 2NO(g) + Cl2(g), Kc = 1.6 x 10− 5 . What...
1. For the reaction: 2NOCl(g) 2NO(g) + Cl2(g), Kc = 1.6 x 10− 5 . What are the equilibrium concentrations of each species if 1.0 mole of NOCl is initially placed in an empty 2.0 L flask? 2. A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H2(g) + I2(g): When the system comes to equilibrium at 425 °C, PHI = 0.708 atm and 2 2 P P H I =...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT