num.. OD D 1/5 Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 5,0 L flask with 1.0 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.25 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. K = | Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use| Privacy Center Acces dtv 23 MacBook Air DII 888 FS esc F2 F3 F4 23 24 7 4 T Y W

The temperature dependence of the equilibrium constant is given by the equation: K- Ae Where K = equilibrium constant T= temperature A = pre-exponential constant factor AH" = standard enthalpy change Use the rules for logarithms and exponents to write this equation in logarithmie form. NOTE: Wite AH as dH (with no spaces) for the answers below. Use ^(caret) to enter superscripts. Submit Answer Retry Entire Group No more group attempts remain

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 6.1 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 3.7 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. Check Explanation Access O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy MAR 28 MacBook Air

Consider the equilibrium N₂O4(g) = 2NO₂(g). At 500 °C, the equilibrium mixture contained 3.86 M nitrogen dioxide gas. Calculate the equilibrium concentration of dinitrogen tetroxide if Kc at this temperature is 0.847. Provide your answer to two places after the decimal and without units. Type your answer...

20 <. At a certain temperature, 0.940 mol SO, is placed in a 2.50 L container. 2 SO, (g) =2 SO, (g) + 0,(g) At equilibrium, 0.140 mol O, is present. Calculate Ke. K. = 2.7738 x10-2 Incorrect help about us privacy policy terms of use careers contact us O Bi w

Q1) For the equilibrium: A B, if [A].0.569, [B].0.162, and Kea 47.8, what are [A]es and [B]ea? algebraic expression: [A]eq= Q2) For the equilibrium: 1221, if [2]. 1.26, [1].0, and Keq = 1.14 x10, what are [12]eg and [lleg? E algebraic expression: [H₂leq_ [12]eg [B]ea. algebraic expression: [12]ea. [eq M Q3) For the equilibrium: H₂ + 1₂2H1, if [H₂lo=0.546, [b]o 1.26, [HI].0, and Kea 45.3, what are [Halea, [lzles and [HI]eq? =0 [HI] eq = 0 0

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.79 at a certain temperature. If a reaction mixture initially contains 0.050 M H2S and 0.050 M SO2, what will the equilibrium concentration of H2O be? 2 H2S(g) + SO2(g)=3 S(s) + 2 H20(g) 1 NEXT > Based on the given values, set up ICE table in order to determine the unknown. 2 H2S(g) SO2(g) 3 S(s) 2 H20(g) + + Initial (M) |Change | (M) Equilibrium | (M) 5 RESET 0.050 +x +2x +3x -x -2x -3x 0.050 + x 0.050 + 2x 0.050 + 3x 0.050 - x 0.050 - 2x 0.050 -3x 0.025 + x 0.025 + 2x 0.025 + 3x 0.025 - x 0.025 - 2x 0.025 -3x

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Part 4 and further example please

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