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The equilibrium constant () of the reaction below is K-6.0 x 10 with initial concentrations as...
Can someone please show me the steps and how to do this problem? Consider the chemical reaction: N2 + 3H2 yields 2NH3. If the concentration of the reactant H2 was increased from 1.0 x 10-2 M to 2.5 x 10-1 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K.
My lab partner and I are both getting different answers for this questions. Can someone please help? If the concentration of the product NH3 was increased from 1.0 x 10-4 M to 5.6 x 10-3 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K.
The following reaction has an equilibrium constant, Kc, of 1.80 x 10-4 at a particular temperature: 2NOCl (g) → 2 NO (g) + Cl2 (g) You have a container in which the concentration of HOCl is 0.99 M, the concentration of NO is 0.45 M, and the concentration of Cl2 is 0.67 M. (a) Calculate the value of the reaction quotient Q. (b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed...
At equilibrium 12(g) + Br2(g) + 2 IBr(g), K = 1.2 x 102 The following concentrations were determined at a particular time: 12(g) = 0.310 mol/L, Br2(g) = 0.310 mol/L and IBr(g) = 2.00 mol/L Calculate Q, the reaction quotient, and by comparing to the K value state if the system is at equilibrium or which direction it will shift if it is not at equilibrium. [3]
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g)...
A Q=K: the reaction mixture is at equilibrium O T OM B. Q<K; the reaction will shift towards the reactants C. Q>K; the reaction will shift towards the products → KA А е е D. Q>K; the reaction will shift towards the reactants MOL (E. Q<K; the reaction will shift towards the products. M280. 00 3. For the reaction M SES00.0 3 to noiriwa H2 (9)+CO2(9) <==> H20 (9) +CO (9) Kc = 0.798 at 320°C. 0.492 moles of H2...
8. In the reaction A products the initial concentration of A is 0.52M and the concentration is 0.12 M after 150.0 min. What is the value of the rate constant, k, in M min'? What is the half-life? k=0.0027 M min"!, t12=97.5 min 9. Consider the following reaction: N2(g) + 3H2(g) + 2NH3(g) (K = 2.41x 10-3) Given 2.00 mole of N2(g), 4.5 mole of H2(g), and 1.5 mole of NH3(g) are mixed in a 5.00 L flask, determine the...
36) At a certain temperature a reaction has K = 2.06 x 101. If all four gases have an initial concentration of 0.800M, what are the equilibrium concentrations? x = change in concentration. Choose all the correct answers. SO3 (g) + NO (g) <--> SO2 (g) + NO2 (g) (Select 6)(6pts) O [SO3) = [NO] = 1.101 M x=0.454 O Q = 1.0 [SO2] = [NO2] = 0.499 M OK=[SO3][NOJ/ [S02] - [NO2] [SO3] = [NO) = 0.499 M O...
(10pts) The equilibrium constant, K, is 2.4 x 10' at a certain temperature for the reaction : 2NO2艹Nao + O20 6. For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift? a) A 1.0-Lflask contains 0.024 mol NO, 2.0 mol Na, and 2.6 mol O b) A 2.0-L flask contains 0.032 mol NO, 0.62 mol N, and 4.0 mol O c) A 3.0-L...
22. A process has an equilibrium constant K of 2.5 x 10' at 300 K. What is AGⓇ at that temperature? A) 19.5 kJ/mol B) 25 kJ/mol C) -19.5 kJ/mol D) 75 kJ/mol 23. In heterogeneous catalysis, the catalyst and reactants are in A) the same B) different C) gaseous phases. D) liquid 24. If the reaction quotient Q. is smaller than K, the reaction will proceed A) to produce more product B) to produce more reactant C) nowhere D)...