Choose the equilibrium expression for the following reaction.a. CH4 (9) + 2H₂S(9) ⇒ CS₂ (9) + 4H₂ (9)OK:=K=OK=K=b. 4NH3(g) + 5O2(g) — 4NO(g) + 6H₂O(g)[NO] 4 [H₂0]6[NH,][0₂]5[NO] [H₂ O]2[NH3][0₂][NO]¹ [H₂O]6[NH₂] 4[NO] ¹ [H₂O]6[NH₂] 4 [0₂]5c. CO₂(g) + MgO(s) = MgCO3(s)OK:OK=OK:OK=K:K=OK=[CS₂] [H₂]4[CH₂] [H₂S][CS₂][CH][H₂S]²[CS₂] [H₂][CH₂] [H₂S]²[CS₂] [H₂] 4[CH₂] [H₂S]²K=1[CO₂][MgCO₂]²[CO₂][MgO][MgCO3][CO₂]²[MgO]²[MgO][CO₂][MgCO3]

In the given reaction, we have to find equilibrium constant (k). x Reactant -----> y Product…

Choose the equilibrium expression for the following reaction. a. CH4 (9) + 2H₂S(9) ⇒ CS₂ (9) + 4H₂ (9) OK: = K= OK= K= OK: b. 4NH3(g) + 5O2 (g) ⇒ 4NO(g) + 6H₂O(g) [NO]¹ [H₂O]6 [NH,][0₂]5 [NO] [H₂ O] 2 [NH3][0₂] OK= OK: [NO]¹ [H₂O]6 [NH₂] 4 [NO] ¹ [H₂O]6 [NH₂] 4 [0₂]5 c. CO₂(g) + MgO(s) = MgCO3 (8) OK= K: K= [CS₂] [H₂]¹ [CH₂] [H₂S] [CS₂] [CH₂][H₂S]² [CS₂] [H₂] OK= [CH₂][H₂S]² [CS₂] [H₂] 4 [CH₂] [H₂S]² OK= 1 [CO₂] [MgCO₂]² [CO₂][MgO] [MgCO3] [CO₂]²[MgO]² [MgO] [CO₂] [MgCO3]

Choose the equilibrium expression for the following reaction. a. CH4 (9) + 2H₂S(9) ⇒ CS₂ (9) + 4H₂ (9) OK: = K= OK= K= OK: b. 4NH3(g) + 5O2 (g) ⇒ 4NO(g) + 6H₂O(g) [NO]¹ [H₂O]6 [NH,][0₂]5 [NO] [H₂ O] 2 [NH3][0₂] OK= OK: [NO]¹ [H₂O]6 [NH₂] 4 [NO] ¹ [H₂O]6 [NH₂] 4 [0₂]5 c. CO₂(g) + MgO(s) = MgCO3 (8) OK= K: K= [CS₂] [H₂]¹ [CH₂] [H₂S] [CS₂] [CH₂][H₂S]² [CS₂] [H₂] OK= [CH₂][H₂S]² [CS₂] [H₂] 4 [CH₂] [H₂S]² OK= 1 [CO₂] [MgCO₂]² [CO₂][MgO] [MgCO3] [CO₂]²[MgO]² [MgO] [CO₂] [MgCO3]

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

Consider the following reaction: 2CO (g) + O2 (g) ⇒ 2CO2 (g). In a 2.00 L vessel, 0.5 moles of carbon monoxide gas reacts with 0.5 moles of oxygen gas. Given that K = 2.2 × 10-22, what are the concentrations of all species at equilibrium? The concentration of CO at equilibrium is The concentration of O2 at equilibrium is The concentration of CO2 at equilibrium is
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?
MOving to anotrie question will save this response. Question 7 A state of dynamic equilibrium, Ag2CO3(s) +→ 2Ag*(aq) + CO32(aqg), exists in solutida. Which direction will the equilibrium shift if Ca(NO3)2(aq) is added to the system? O To the left. O To the right. O It will not shift left or right. A Moving to another question will save this response. MacBook Pro 80 888 FS F6 F7 FA esc F2 %23 2$ 8. 2 3 4. Q K A D 5
A 75.0 g sample of a pure liquid, liquid A, with a density of 3.00 g/mL is mixed with a 50.0 mL sample of a pure liquid, liquid B, with a density of 2.00 g/mL. What is the total volume of the mixture? (Assume there is no reaction upon the mixing of A and B and volumes are additive.) O a. 175 mL O b. 75.0 mL O c. 125 mL O d. 275 mL O e. 100. mL
Consider the following reaction and its equilibrium constant at some temperature. 2NH3(g) = N₂(g) + 3H₂(g) K₂=35 If the following concentrations are present initially: [NH3] = 0.10 M; [N₂] = 2.00 M; [H₂) = 2.00 M.. Which of the following is correct about the reaction? 1.The reaction is at equilibrium. 2.The reaction is not at equilibrium, it will shift to the left to reach equilibrium. 3.the reaction is not at equilibrium it will shift to the right to reach equilibrium.
Please help with question 1
Consider the following reaction at equilibrium. What effect will removing some SO2 have on the system? SO2(g) + NO2(g) = SO3(g) + NO(g) The pressure of SO3 will increase The equilibrium constant will decrease. No change will occur since SO2 is not included in the equilibrium expression. The pressure of NO2 will increase. The reaction will shift to decrease the pressure.
Write the equilibrium expression for 2NO(g) + 2H2(g) = N2(g) + 2H20(g). a. Ke = [H20]2 [N2] / [NO]² [H2]² O b. Kc [N2]/ [NO]2 [H2]? %3D O c. Ke [NO]? [H2]? / [H2O]² [N2] %3D
Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 5.40x10-4 moles of NH3(g), 0.450 moles of N₂, and 0.215 moles of H₂ are at equilibrium in a 15.1 L container at 846 K, the value of the equilibrium constant, K, is
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N₂(g) + 2 H₂O(g) 2 H₂(g) + 2NO(g) = -9 K₂=3.x 107 He fills a reaction vessel at this temperature with 15. atm of nitrogen gas and 7.8 atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NO, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NO at right. Round your answer to 1 significant digit. O yes O no 0 atm 0 10 X