Consider the following reaction: NH4HS(s)⇌NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was...

Question

Question

Consider the following reaction: NH4HS(s)⇌NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was...

Consider the following reaction:

NH4HS(s)⇌NH3(g)+H2S(g)

An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]= 0.284 M and [H2S]= 0.355 M.

You may want to reference (Pages 651 - 653) Section 15.6 while completing this problem.

Part A

What is the value of the equilibrium constant (Kc) at this temperature?

science chemistry

Add a comment Improve this question Transcribed image text

Answer 1

Answer #1

Equilibrium constant = [NH3] [H2S] , it is Expressed as the ratio of concentration of product to that of reactants raised to the power that is the stoichiometric coefficient , substitution of the value ,we get Kc = 0.1008

Add a comment

Answer 2

Similar Homework Help Questions

Consider the following reaction: NH4HS(s)⇌NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was...

Consider the following reaction: NH4HS(s)⇌NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was found to have [NH3]= 0.280 M and [H2S]= 0.355 M . What is the value of the equilibrium constant (Kc) at this temperature?
Consider the reaction: NH4HS (s) <--> NH3 (g) + H2S (g)

Consider the reaction: NH4HS (s) <--> NH3 (g) + H2S (g). An equilibrium mixture of this reaction at a certain temperature was found to have [NH3] = 0.278 M and [H2S] = 0.355 M. What is the value of the equilibrium constant (Kc) at this temperature? a. 0.126 b. 0.355 c. 0.783 d. 0.0987 e. 0.278
an equilibrium mixture of this reaction at a certain temperature was found to have [NH3]=0.290 M...

an equilibrium mixture of this reaction at a certain temperature was found to have [NH3]=0.290 M and H2S =0.370 M. what is the valur of the equilibrium constant (Kc) at this temperature? Exercise 14.36 Consider the following reaction: equilibrium mixture of this reaclion at a certain temperature was found to have NHa 0290 M and H S 0.370 M

The equilibrium constant, K, for the following reaction is 0.186 at 332 K. NH4HS(s) (equilibrium) NH3(g)...

The equilibrium constant, K, for the following reaction is 0.186 at 332 K. NH4HS(s) (equilibrium) NH3(g) + H2S(g) An equilibrium mixture in a 16.2 L container at 332 K contains 0.322 mol NH4HS(s), 0.543 M NH3 and 0.343 M H2S. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 8.20 L? [NH3] = M [H2S] = M
Consider this reaction: NH, HS(8) NH3(g) + H2S(9) An equilibrium mixture of this reaction at a...

Consider this reaction: NH, HS(8) NH3(g) + H2S(9) An equilibrium mixture of this reaction at a certain temperature was found to have (NH3) = 0.258 M and (H2S) = 0.315 M. Part A What is the value of the equilibrium constant at this temperature? Express your answer to three significant figures. | ΑΣφ ? Kog Submit Request Answer < Return to Assignment Provide Feedback
Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction NH4HS(s)⇌NH3(g)+H2S(g) This reaction...

Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction NH4HS(s)⇌NH3(g)+H2S(g) This reaction has a Kp value of 0.120 at 25 ∘C. What are the partial pressures of NH3 and H2S at equilibrium, that is, what are the values of PNH3and PH2S, respectively? Enter the partial pressure of ammonia followed by the partial pressure of hydrogen sulfide numerically in atmospheres separated by a comma. What is the mole fraction, χ, of H2S in the gas mixture at...

The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g)...

The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 5.41 L container at 548 K contains 1.17 mol of NH4Cl(s) and 0.350 mol of NH3, the number of moles of HCl present is ( ) moles. The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g) If an equilibrium mixture of the three...
a) The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g)...

a) The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g) Calculate the equilibrium concentration of H2S when 0.318 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] = _____M b) The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.313 moles of COCl2(g) are introduced into a 1.00 L vessel...
Constants 1 Pe Consider the reaction between NO and Cl2 to form NOCI: 2NO (g) +...

Constants 1 Pe Consider the reaction between NO and Cl2 to form NOCI: 2NO (g) + Cl2 (g) = 2NOCl (9) A reaction mixture at a certain temperature initially contains only (NO) = 0.67 Mand (Cl2] = 0.55 M . After the reaction comes to equilibrium, the concentration of NOCI is 0.34 M. Part A You may want to reference (Page 688) Section 15.6 while completing this problem. Find the value of the equilibrium constant (Kc) at this temperature. Express...

The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) H3(g) +H2S(g)...

The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) H3(g) +H2S(g) Calculate the equilibrium concentration of H2S when 0.261 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] =

Consider the following reaction: NH4HS(s)⇌NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was...

Homework Answers

Add Answer to:
Consider the following reaction: NH4HS(s)⇌NH3(g)+H2S(g) An equilibrium mixture of this reaction at a certain temperature was...

Post as a guest

Earn Coins