NH4HS(s) ⇌ NH3(g) + H2S(g) At a certain temperature, Kc = 8.5 x10^-3. For a reaction...
NH4HS(s) ⇌ NH3(g) + H2S(g)
At a certain temperature, Kc = 8.5 x10^-3. For a reaction mixture at this temperature containing solid NH4HS and the following concentrations of NH3(g) and H2S(g), will more solid form, or will some of the existing solid decompose as equilibrium is reached?
| [NH3] = 167 mM | [H2S] = 51 mM | more solid | solid decomposes | no change |
| [NH3] = 125 mM | H2S] = 58 mM | more solid | solid decomposes | no change |
| [NH3] = 220 mM | [H2S] = 12 mM | more solid | solid decomposes | no change |
| [NH3] = 76 mM | [H2S] = 135 mM | more solid | solid decomposes | no change |
Homework Answers
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NH4HS(s) ⇌ NH3(g) + H2S(g)
At a certain temperature, Kc = 8.5 x10^-3. For a reaction...
27. Consider the reaction. NH,HS(s) NH3(g) + H2S(g) At a certain temperature, Ke-8.5 × 10-3 In...
27. Consider the reaction. NH,HS(s) NH3(g) + H2S(g) At a certain temperature, Ke-8.5 × 10-3 In a reaction mix- ture at this temperature containing solid NH,HS INH3] 0.166 M and [H S] 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?
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 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?
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
The reaction CO2(g) + C(s) <-> 2CO(g) has a Kp=5.78 at 1200k Delta n for the...
The reaction CO2(g) + C(s) <-> 2CO(g) has a Kp=5.78 at 1200k Delta n for the reaction is ___ Kc for the reaction is ____ 2) For the following reaction:NH4HS(s)<->NH3(g) + H2S (g) Kc=8.5x10^-3 At any given point the reaction mixture has solid NH4HS, NH3 at 0.166M and H2S at 0.166M. Is the reaction at equilibrium? Will more of the solid form, or will some of the existing solid decompose? 3) Consider the following reaction: CH3OH (g) <-> CO (g)...
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, 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
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...
The reaction NH4HS(s) ⇌ NH3(g) + H2S(g) has Kc = 1.8 x 10–4 at 25°C. If...
The reaction NH4HS(s) ⇌ NH3(g) + H2S(g) has Kc = 1.8 x 10–4 at 25°C. If excess NH4HS(s) is allowed to equilibrate at 25°C, what is the equilibrium concentration of NH3? A) 3.2 x 10–8 M B) 9.0 x 10–5 M C) 1.8 x 10–4 M D) 6.7 x 10–3 M E) 1.3 x 10–2 M
1) For the following reaction: SO2Cl2(g)<-> SO2(g) + Cl2 (g) Kp=2.91x10^3 at 298K In the reaction...
1) For the following reaction: SO2Cl2(g)<-> SO2(g) + Cl2 (g) Kp=2.91x10^3 at 298K In the reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of CL2 is 285 torr. The partial pressure of SO2Cl2 is [x]torr. 2) For the following reaction:NH4HS(s)<->NH3(g) + H2S (g) Kc=8.5x10^-3 At any given point the reaction mixture has solid NH4HS, NH3 at 0.166M and H2S at 0.166M. a) Is the reaction at equilibrium? b)Will more of the solid form, or will...
27. Consider the reaction. NH,HS(s) NH3(g) + H2S(g) At a certain temperature, Ke-8.5 × 10-3 In a reaction mix- ture at this temperature containing solid NH,HS INH3] 0.166 M and [H S] 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?
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