Question

What will be the shift in equilibrium for each of the following reactions upon increasing the...

What will be the shift in equilibrium for each of the following reactions upon increasing the temperature?

a) N​2(g) + 3H2(g) ​<----> 2NH3(g)         ​deltaH= -92.38kJ

b) N​2(g) ​+ O2(g)​ <----> 2NO(g)​        deltaH= 90.3kJ

c) CO(g) + H​2O​(g) <-----> CO​2(g) ​+H2(g) ​      deltaH= -41.16kJ

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
Would increasing the volume of the container for each of the following reactions at equilibrium cause...
Would increasing the volume of the container for each of the following reactions at equilibrium cause the system to shift in the direction of the products or the reactants? Part A 2NH3(g)???3H2(g)+N2(g) A. Increasing the volume will shift the system in the direction of the products. B. Increasing the volume will shift the system in the direction of the reactants. C. Increasing the volume will not shift the equilibrium. Part B N2(g)+O2(g)???2NO(g) A. Increasing the volume will shift the system...
Determine how each of the following changes will affect the equilibrium reaction below (shift left, shift...
Determine how each of the following changes will affect the equilibrium reaction below (shift left, shift right, no change) H2O(g) + C(s) ↔ H2(g) + CO(g) ∆H° = 131 kJ a. increasing the temperature b. adding CO c. removing H2 c. removing H e. increasing the volume of the container f. adding more carbon to the reaction
What would be the effect of increasing the volume on each of the following reactions at...
What would be the effect of increasing the volume on each of the following reactions at equilibrium (shift left, shift right, or no change)? A) 2CO (g) + O2 (g) <-----> 2CO2 (g) B) N2O4 (g) <-----> 2NO2 (g)
Assuming that each of the following reversible reactions has reached a state of equilibrium, indicate with...
Assuming that each of the following reversible reactions has reached a state of equilibrium, indicate with an arrow, showing direction of shift, the effect of each change upon the equilibrium. Assume that only one change is made at a time. a) 2 Cl2(g) + 2 H2O(g) + heat  4 HCl(g) + O2(g) (1) Raise P (2)Raise T b) Fe2O3(s) + 3 H2(g)  3 H2O(g) + 2 Fe(s) (1) Add Fe(s) (2) Raise P c) 2 NH3(g) + heat...
Using the information below determine the change in enthalpy for the following reaction:             2NO(g) +...
Using the information below determine the change in enthalpy for the following reaction:             2NO(g) + 5 H2(g) → 2NH3(g) + 2H2O(l) H2(g) + ½ O2(g) →   H2O(l)                     ∆H°= -285.8kJ N2(g) + O2(g)   → 2NO(g)                     ∆H°= +180.5 kJ 2NH3(g) → N2(g) + 3H2(g)                    ∆H°= + 92.22 kJ please explain step by step! thanks!
1.         Write equilibrium (mass action) expressions for each of the following reactions: (a) H2(g) + I2(g)          2 HI...
1.         Write equilibrium (mass action) expressions for each of the following reactions: (a) H2(g) + I2(g)          2 HI (b)2 NO(g) + O2(g)           2 NO2(g) (c)N2(g) + 3 H2(g)           2 NH3(g) (d) CO(g) + NO2(g)           CO2(g) + NO(g) (e) 2 CO(g) + O2(g)             2 CO2(g) 2.    Write equilibrium expressions for each of the following equilibria: (a) 2 C(s) + O2(g)                  CO(g) (b) Zn2+(aq) + H2S(g)               ZnS(s) + 2 H+(aq) (c) HCl(g) + H2O()                  H3O+(aq) + Cl–(aq) (d)H2(g) +  O2(g)                   H2O(g) 3.         Which of the following is more likely to precipitate the hydroxide ion? (a)...
Determine the direction in which equilibrium will be shifted by the following changes. (Answers can be:...
Determine the direction in which equilibrium will be shifted by the following changes. (Answers can be: shift to products, shift to reactants, no change) N2(g) + 3H2(g) ⇌ 2NH3(g) (This reaction is exothermic and requires a catalyst to occur readily.) a. Increasing [N2]   ______________________________________________ b. Increasing pressure ______________________________________________ c. Decrease in temperature ______________________________________________
For each of the following reactions, predict the effect of increasing pressure will have on each...
For each of the following reactions, predict the effect of increasing pressure will have on each of the following reactions at equilibrium. Assume that temperature is constant but that pressure changes are obtained by changing the volume of the container.       -       A.       B.       C.       D.    2A(s) ⇌ B(s)       -       A.       B.       C.       D.    A(l) ⇌ 2B(l)      ...
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...
Based on the standard free energies of formation, which of the following reactions represent a feasible...
Based on the standard free energies of formation, which of the following reactions represent a feasible way to synthesize the product? A. N2(g)+H2(g)→N2H4(g); ΔG∘f=159.3 kJ/mol B. N2(g)+3H2(g)→2NH3(g); ΔG∘f=−33.30 kJ/mol C. N2(g)+O2(g)→2NO(g); ΔG∘f=173.2 kJ/mol D. 2SO(g)+O2(g)→2SO2(g); ΔG∘f=−600.4 kJ/mol Drag the appropriate items to their respective bins. feasible synthesis- not a feasible synthesis-
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT