6. Considering the following system at equilibrium:AH =+ 215 kJC.H.(g) + Cl:(g)= C;H;Cl:(g)AH = - 215 kJa. If CH4 is added:i. Will equilibrium shift to the left or the right?ii. What happens to the concentration of Cl2?iii. What happens to the concentration of C2H;Cl2?b. If Cl2 is removed:i. Will equilibrium shift to the left or the right?ii. What happens to the concentration of C,H,?iii. What happens to the concentration of CH;Cl2?c. If the temperature is increased:i. Will equilibrium shift to the left or the right?ii. What happens to the concentration of Cl2?iii. What happens to the concentration of C,H,?iv. What will happen to the concentration of C¿H¿Cl2?d. If the pressure is increased:i. will equilibrium shift to the left or the right?ii. What happens to the concentration of Cl2?iii. What happens to the concentration of C,H,?iv. What will happen to the concentration of CH2C12?

Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Considering the following system at equilibrium: AH =+ 215 kJ AH = - 215 kJ %3D CH(g) + Cl:(g)2 C,H;Cl;(g) a. If C;H4 is added: i. Will equilibrium shift to the left or the right? ii. What happens to the concentration of Cl2? iii. What happens to the concentration of C2H½CI2? b. If Cl2 is removed: i. Will equilibrium shift to the left or the right? ii. What happens to the concentration of C,H,? iii. What happens to the concentration of C2H2CI2? c. If the temperature is increased: i. Will equilibrium shift to the left or the right? ii. What happens to the concentration of Cl2? iii. What happens to the concentration of C,H,? iv. What will happen to the concentration of CH;Cl2?

Considering the following system at equilibrium: AH =+ 215 kJ AH = - 215 kJ %3D CH(g) + Cl:(g)2 C,H;Cl;(g) a. If C;H4 is added: i. Will equilibrium shift to the left or the right? ii. What happens to the concentration of Cl2? iii. What happens to the concentration of C2H½CI2? b. If Cl2 is removed: i. Will equilibrium shift to the left or the right? ii. What happens to the concentration of C,H,? iii. What happens to the concentration of C2H2CI2? c. If the temperature is increased: i. Will equilibrium shift to the left or the right? ii. What happens to the concentration of Cl2? iii. What happens to the concentration of C,H,? iv. What will happen to the concentration of CH;Cl2?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

at 200 ° C, the numerical value of Kc for the following reaction is 8 × 10-³. PCl5 = PCl3 + Cl2 deltaH = + 124 kj / mol a) How would it affect the value of the equilibrium constant if: i.add PCl5 ii.pressure increases iii.the temperature rises.
For each organic reaction, say whether at equilibrium there will be more reactants than products (so equilibrium lies ro the left), or more products than reactants (so equilibrium lies to the right)...
K=4.9x10-3 for the reaction CO₂(g)+H₂(g)⇒ CO(g)+H₂O(g). If [CO₂]=0.00025 M, [H₂]=0.0010 M, & [CO]=0.000015 M, what is the concentration at equilibrium of H₂O? 1.8x10-14M 8.2x10-5M 0.29 M 3.4 M
MISSED THIS? Read Section 16.6 (Page); Watch IWE 16.5. Consider the following reaction: SO₂ Cl2 (g) SO2 (g) + Cl2 (g) A reaction mixture is made containing an initial [SO₂ C1₂] of 2.0×10-² M . At equilibrium, [Cl₂] = 1.1×10-² M. Part A Calculate the value of the equilibrium constant (Kc). Express your answer to two significant figures. for Part A for Part A do for Part redo fol Part A reset for Part. Ke= 2.2410-² Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
Consider the reaction: S(s) + O2(g); SO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ką and K,, for reactions a and b below: а.) 2 S(8) + 3 О2(g) 2 SO3(g) Ka b.) SO2(g) + 1/2 02(g) SO3(g) K, K =
What will happen to the NO concentration at equilibrium if the [NO2] is raised NO2(g) NO(9) + N203(9) energy + A. increase B. decrease O C. stay the same
How will the equalibrium shift? Heat + N2 (g) + 3O2 (g) <----> 2NO (g) a) how will it shift with an addition of NH3 b) how will it shift with increase in pressure?
1. What is the equilibrium constant expression Kc, for the following balanced equation? 2|NH3] 3 N2]H2] а. [N2][H2]3 [NH3]² 3 N2]H2] 2[NH3] С. NH3]2 [N2][H2]³ d.
Tim Express the equilibrium constant for the following reaction. N2(8) +3 H2(g) = 2 NH3(g) Select one: N2][H2P K = NH3P O A. [N2]H2]!/3 K = NH3]12 O B. NH3]/2 K = N2][H2]!/3 OC. OD. K = N2[H23 NH3P O E. NH36 K = N2PH2P AGE FINISH ATTEM TOSHIBA B/O 144 24 &
It is A or C because im really confuse right now i thought pure liquid is not included in equilibrium so what is the right answer please help me to know if
Consider the following system at equilibrium at 800 K:2H2(g) + S2(g) = 2H2S(g) + 69.3 kcalIf the TEMPERATURE on the equilibrium system is suddenly increased: The reaction must: A. Run in the forward direction to reestablish equilibrium. B. Run in the reverse direction to reestablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of S2 will: A. Increase. B. Decrease. C. Remain the same.
Consider the reaction: C(s) + O2(g)CO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K, and K,. for reactions a and b below: a.) C(s) + 1/2 O2(g) Co(g) Ka b.) CO(g) + 1/2 O2(g): Co2(g) K, K=