.170 grams of ammonia was placed in a 2-liter round flask at a
temperature of 25 C. Determine the pressures of each gas after
reaching equilibrium.
NH4HS(s) -----> HG3(g) + H2S(g)
<-----
Kp=.108 at 25 degrees C
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
.170 grams of ammonia was placed in a 2-liter round flask at a temperature of 25...
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 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 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)
please show all work thanks B. Consider the system N2 (9) 3H2 (g) 2 NHs (9) dbie of NHs was placed in a 2.000 liter flask at 25°C. When equilibrium at that temperature, it was determined that the ammonia was reduced A 2.568-g sample was reached N to 75.0% of its original value. 1. Calculate K for the decomposition of 2.00 moles of ammonia at 25.0°C. 2. Calculate K for the decomposition of 2.00 moles of ammonia at NH3 is...
(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...
30. A 5.71 gram sample of PCi5 is placed in an evacuated 1.8 liter flask at 264°C and decomposes to phosphorus trichloride and chlorine gas. (a) Write the balanced equation for the decomposition reaction of PCi5. (b) Calculate the initial pressure in the flask before the PC15 decomposed, (c) If 75% of the PC15 decomposes, calculate the partial pressures of all three gases in the flask after the reaction is completed.
16.) Nitrosyl bromide, , dissociates readily at room temperature. Some is placed in a flask at 25 °C and allowed to dissociate. The total pressure at equilibrium is 130 mm Hg and the compound is found to be 37% dissociated. What is the value of Kp?
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 5.0 L flask with 1.3 atm of ammonia gas at 46. °C . He then raises the temperature, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.39 atm . Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. kp=_______
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 5.0 L flask with 1.3 atm of ammonia gas at 46. °C . He then raises the temperature, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.39 atm . Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. kp=_______
The equilibrium below is established by placing solid NH4HS in an evacuated container at 25 0C. At equilibrium, some solid NH4HS remains in the container. NH4HS(s) « NH3(g) + H2S(g) delta H0 = +93 kilojoules Predict and rationalize, using LCP only, each of the following. The effect on the equilibrium partial pressure of NH3 gas when additional solid H2S is introduced into the container. The effect on the mass of solid NH4HS present when the volume of the container...