Dinitrogen tetroxide partially decomposes according to the following equilibrium: N2O4 (g) →2NO2 (g) A 1.000-L flask is charged with 1.00 ⋅⋅ 10-2 mol of N2O4. At equilibrium, 6.61 ⋅ 10-3 mol of N2O4 remains. Keq for this reaction is ________. A. 0.207 B. 6.94 ⋅ 10-3 C. 3.39 ⋅ 10-5 D. 0.203 E. 0.212

Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed?  a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases

Consider the following equilibrium reaction: 2F + H₂O + CO2(g) Predict which direction the equilibrium will shift (left, towards reactants or right, towards products) when you perform the following actions: i) A+ 2HF, + CO²- (aq) 3(aq) ii) Action Add HF to the reaction Add Na₂CO3 to the reaction Add NaCl Add KF to the reaction Add CO₂ to the reaction Remove CO₂ from the reaction Remove HF from the reaction Increase pressure by reducing volume Cool the reaction mixture Heat the reaction mixture Provide four suggestions to increase the amount of CO₂ gas generated. iv) Shift Left Shift Right

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide?5N2O4(g) ----><----- 10NO2 (g) A. [N2O4] 5 /[NO2] 5 B. [NO2] 5 /[N2O4] 10 C. [N2O4] 10 /[NO2] 5 D. [NO2] 5 /[N2O4] 5 E. [NO2] 10 /[N2O4] 5

A. Write the equilibrium expression or the chemical equation of the following reactions and calculate its equilibrium constant. 1. 2 Ag2CO3(s) 4 Ag + 2 CO2(g) + O2(g) 2. H2O(g)_ + C(s) → CO(g) H2(2) [HI?] 3. Ke [H2][I2] [03]? K.= [02]3 [HCl]2 K.= [Cl2][H2] 5. 4.

4. What is the equilibrium constant expression for the reaction CH4 (s) +2O2 (g) CO2 (g) + 2H2O (l)a. [CO2][H2O]2 / [CH4][O2]2 c. [CO2] / [O2]2b. [CO2][H2O]2 / [O2]2 d. [CH4][O2]2 /[CO2][H2O]2

What is the correct form for the equilibrium constant for this reaction? H2 (g) + F2 (e) = 2HF(e) (g) = 2HF(g) [HE]?- [H2][F2] --IHF]_ [H2][F2] O _[H2][E2]_- [HF] O -_[H2][E2]_ 2[HF]

Which statements are always correct for a reaction at equilibrium? The forward and reverse reactions both continue. The concentrations of reactants and products are equal. The rates of the forward and reverse reactions are equal. I. II. |||. OII and III only I and III only I, II, and III I and II only

For the following chemical reaction, CO(g) + H₂O (g) →CO₂ (g) + H₂ (g) Kc = 0.0257 If a 2.00L vessel is charged with 0.200 moles of CO, 1.13 moles of H₂O, 0.199 moles of CO2, and 0.175 moles of H2, what is the equilibrium concentration of CO? a. 0.264M b. 0.145M O c. 0.0451M O d. 0.054M e. 0.610M

20. What will happen to the equilibrium when more SO2 (g) is added to the following system? 2502(g) + O2(g) = 250(g) A. It will shift to the right. B. It will shift to the left C. no shift of equilibrium D. cannot be determined 21. For the reaction 2A+B2C the appropriate form for the equilibrium constant expression is: A. [A][B12/ [C] B. [AB]/[C12 C. [C]2/[A][B] D. [ABRIC] 22. Calculate K for the following reaction given the following equilibrium concentrations of H2, CO, and H₂O. PCl3(g) + Cl₂(g) K=? Equilibrium Concentrations (M): PCIs(g) .200 .040 .080 A. 0.16 B.0.016 C.1.6 D.16 23. Which of the following is not omitted when writing the equilibrium constant expression? D. all of the choices A. gas C. solid B. liquid 24. When can we say that the reaction is already at equilibrium? A. When Q is not equal to K. C. When Q is greater than K. D. When Q is lesser than K. B. When Q is equal to K. 25. Where will the equilibrium shift when we increase the pressure of the system? B. towards…