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.
| P = | 6.46 |
Homework Answers
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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...
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...
± Heterogeneous Equilibrium of Ammonium Bisulfide - Copy Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen...
± Heterogeneous Equilibrium of Ammonium Bisulfide - Copy 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. An empty 5.00-L flask is charged with 0.300 g of pure H2S(g), at 25 ∘C. Part A What is the initial pressure of H2S(g) in the flask? Express your answer numerically in atmospheres. Hints P = 4.31×10−2 atm SubmitMy AnswersGive Up Correct Addition of ammonium bisulfate In...
3) Ammonium hydrogen sulfide dissociates into ammonia gas and hydrogen sulfide gas in a spooky space ship. If we sta...
3) Ammonium hydrogen sulfide dissociates into ammonia gas and hydrogen sulfide gas in a spooky space ship. If we start with a sample of pure NH4HS(S) at 25°C in a vacuum, the total pressure of the gases is 0.658 atm when equilibrium is established. Determine the value of Kp NH4HS($) + NH3(g)+H2S(g)
100 g of solid ammonium hydrogen sulfide (NH4HS) was introduced into an empty 1.0 L reaction...
100 g of solid ammonium hydrogen sulfide (NH4HS) was introduced into an empty 1.0 L reaction vessel. The closed vessel was heated to 300 o C, and the following reaction came to equilibrium: NH4HS(s) ⇌ NH3(g) + H2S(g) At equilibrium, the total pressure inside the reaction vessel was 0.9 atm. Calculate the value of Kp for this reaction.
Enter your answer in the provided box. Ammonium hydrogen sulfide decomposes according to the following reaction,...
Enter your answer in the provided box. Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp = 0.11 at 250°C: NH4HS(S) = H2S(g) + NH3(g) If 53.1 g of NH4HS() is placed in a sealed 5.0-L container, what is the partial pressure of NH3(g) at equilibrium? Рун, = atm
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
(a) Consider the following reaction NH4HS(S) NH3g) H2S(g) For this reaction Kp 0.05 atm2 at 20 C. In a particular experiment, 0.06 mole of solid NH4HS is introduced into a 2.4 dm3 flask at 20 '...
(a) Consider the following reaction NH4HS(S) NH3g) H2S(g) For this reaction Kp 0.05 atm2 at 20 C. In a particular experiment, 0.06 mole of solid NH4HS is introduced into a 2.4 dm3 flask at 20 'C. Assume that the gases are ideal. Given: R 0.082 atm dm3 K-1 mol-1: R 8.314J K-1 mol-1 (i) Calculate the percent of the solid that will have decomposed at equilibrium (ii)Calculate the number of moles of ammonia that would have to be added to...
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) NH3(g) +...
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) NH3(g) + H2S(g) If ΔH° for this reaction is 92.7 kJ, what is the value of Kp at 212 K? Kp =
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?
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
3) Ammonium hydrogen sulfide dissociates into ammonia gas and hydrogen sulfide gas in a spooky space ship. If we start with a sample of pure NH4HS(S) at 25°C in a vacuum, the total pressure of the gases is 0.658 atm when equilibrium is established. Determine the value of Kp NH4HS($) + NH3(g)+H2S(g)
Enter your answer in the provided box. Ammonium hydrogen sulfide decomposes according to the following reaction, for which Kp = 0.11 at 250°C: NH4HS(S) = H2S(g) + NH3(g) If 53.1 g of NH4HS() is placed in a sealed 5.0-L container, what is the partial pressure of NH3(g) at equilibrium? Рун, = atm
(a) Consider the following reaction NH4HS(S) NH3g) H2S(g) For this reaction Kp 0.05 atm2 at 20 C. In a particular experiment, 0.06 mole of solid NH4HS is introduced into a 2.4 dm3 flask at 20 'C. Assume that the gases are ideal. Given: R 0.082 atm dm3 K-1 mol-1: R 8.314J K-1 mol-1 (i) Calculate the percent of the solid that will have decomposed at equilibrium (ii)Calculate the number of moles of ammonia that would have to be added to...
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