A. Write the forward and reverse reactions for e each of the following:a. N2(g) + 3H2(g) <===> 2NH3(g)b. 2C0(g) + 02 <===> 2CO2(g)

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Answered: A. Write the forward and reverse…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the following reaction: 2NH3 (9) N2(g) + 3H₂ (9) = If 0.00148 moles of NH3(g), 0.268 moles of N₂, and 0.643 moles of H₂ are at equilibrium in a 11.7 L container at 932 K, the value of the equilibrium constant, Ke, is
8.2 mol NH3 are placed in a 10.5 L container at some temperature and allowed to come to equilibrium as per the reaction below. At equilibrium, 2.2 moles remained. What is the value of Kc for the following reaction at the temperature of the experiment? 2 NH3(g) N2(g) + 3 H2(g)
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As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C
In which of the following reactions will Kc = Kp? 2 SO3(s) + 2 NO(g) = 2 SO2(3) + 2 NO2(3) 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H2O(g) O 4 N2(3) + 2 O2(g) =4 N20(g) O 6 SO2(g) + 3 O2(3) =6 SO3(g)
For the equilibrium 3NO₂(g) K₂=1.0 x 10-11 N₂O5(g) + NO(g) If a 4.00 L container initially holds 0.25 mol of NO₂, how many moles of N₂O5 will be present when this system reaches equilibrium? Enter your answer in scientific notation. moles of N₂O5 = i x 10 Mi mol
1
Consider the following reaction: ΔΗ, AH'; (-) mol mol K -297 248 2SO₂(g) + O₂(g) → 2503(g) SO₂(g) SO₂(g) -396 257 0₂(g) 0 205 A reaction mixture is prepared at 80.0°C containing 0.30 atm of SO2, 1.00 atm of 0₂, and 8.00 atm of SO3. Calculate AG and AG, both in units of kJ/mol. As always, you must clearly and logically show all of your work Additional information R= 8.3145 J mol K AGAH-TAS AG-RT In(K) AG AG° + RT In(Q) So
2NO(g) + O₂(g) → NO2(g) Conc. NO, mol/L Exp. 1 4.3 x 10-2 Exp. 2 4.3 x 10-2 Exp. 3 8.6 x 10-² Exp. 4 0.63 Conc. 02, mol/L 2.4 x 10-² 4.8 x 10-2 9.6 x 10-² 5.4 x 10-³ Initial Rate 8.0 x 10³ mol/(L.s) 1.6 x 102 mol/(L.s) 0.13 mol/(L.s) ? a What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law = K[NO]²[0₂]✔ Co- The reaction is first order in O₂ because the rate doubled with a do second order in NO because the rate increased by a factor of 8 wh Rate = k[NO] ² [0₂] b What is the initial rate of the reaction in Experiment 4? Initial rate= mol/(L.s)

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A. Write the forward and reverse reactions for e each of the following: a. N2(g) + 3H2(g) <===> 2NH3(g) b. 2C0(g) + 02 <===> 2CO2(g)