QUESTION 1 The equilibrium constant for the reaction 2NOBr(g) = 2NO(g) + Br 2(g) is 6.2 x 10 3 at 300°C. A mixture of gases has the following composition: [NOBr] = 3.5 x 10 3 mol/L, [NO] = 6.5 x 10 3 mol/L, and [Br 2] = 1.9 × 10 3. Is the system at equilibrium? If not, in which direction does the reaction proceed? Yes, the system is at equilibrium. No, products are converted to reactants. No, reactants are converted to products. No, equilibrium cannot be achieved.

QUESTION 1 The equilibrium constant for the reaction 2NOBr(g) = 2NO(g) + Br 2(g) is 6.2 x 10 3 at 300°C. A mixture of gases has the following composition: [NOBr] = 3.5 x 10 3 mol/L, [NO] = 6.5 x 10 3 mol/L, and [Br 2] = 1.9 × 10 3. Is the system at equilibrium? If not, in which direction does the reaction proceed? Yes, the system is at equilibrium. No, products are converted to reactants. No, reactants are converted to products. No, equilibrium cannot be achieved.

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...

See similar textbooks

Similar questions

The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) H₂(g) + 1₂(g) ? An equilibrium mixture of the three gases in a 1.00 L flask at 698 K contains 0.330 M HI, 4.43×10-² M H₂ and 4.43×10-2 M 1₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.69x10-2 mol of H₂(g) is added to the flask? [HI] = [H₂] = [1₂] = ΣΣΣ
The equilibrium constant, Kp, for the following reaction is 1.80×10-2 at 698K.2HI(g) H2(g) + I2(g)If an equilibrium mixture of the three gases in a 10.1 L container at 698K contains HI at a pressure of 1.21 atm and H2 at a pressure of 0.805 atm, the equilibrium partial pressure of I2 is atm --- Consider the following reaction:2NH3(g) N2(g) + 3H2(g)If 4.60×10-4 moles of NH3, 0.234 moles of N2, and 0.205 moles of H2 are at equilibrium in a 15.6 L container at 814 K, the value of the equilibrium constant, Kp, is .
The equilibrium constant, Kp, for the following reaction is 1.04×10-² at 548 K. NH4CI(S)2NH3(g) + HCI(g) If an equilibrium mixture of the three compounds in a 6.72 L container at 548 K contains 1.63 mol of NH4Cl(s) and 0.190 mol of NH3(g), the partial pressure of HCI(g) is I atm.
The equilibrium constant, Kc, for the following reaction is 9.52×10-2 at 350 K:CH4(g) + CCl4(g) 2CH2Cl2(g)Calculate the equilibrium concentrations of reactants and product when 0.368 moles of CH4 and 0.368 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [CH4] = M [CCl4] = M [CH2Cl2] = M
3 H2(g) + N2 (g) the equilibrium For the reaction 2NH3(g) ---- 3H2(g) +N2(g) 2 NH 3 (g) - concentrations were found to be [NH3] = 0.250 M, [H2] = 0.330 M and [N2] = 0.750 M. What is the equilibrium constant for this reaction?
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g)↽−−⇀4C(g) ?c=2.13×10^25 If, at this temperature, 2.30mol of A and 3.60mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A]= M [B]= M [C]= M
In order to study the system at 400 K, 0.50 mol Br2, 0.50 mol Cl2, and 1.0 mol BrCl were added to a 2.0 L container. Br₂(g) + Cl₂(g) = 2BrCl(g) Kc = 7.0 Calculate the concentrations of the reactants and products at equilibrium. What is the concentration of Cl2 at equilibrium? [Cl₂] = [?] x 10 M Coefficient (green) Exponent (yellow) Enter
Some NOBR is placed in a sealed flask and heated to 385 K. When equilibrium is reached, the flask is found to contain NOBR (9.30×103 M), NO (1.27x102 M), and Br2 (1.18×102 M). What is the value of the equilibrium constant for this reaction at 385 K? 2NOBR(g)=2NO(g) + Br2(g) K=
The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COC,(g) CO(g)+ Cl(g) Calculate the equilibrium concentrations of reactant and products when 0.260 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K. [COC,] = [ M [CO] M [Ch] M
A student ran the following reaction in the laboratory at 1171 K: 2502(g) + O₂(g) = 2503(9) When she introduced 7.80 x 10-2 moles of SO₂(g) and 8.76x102 moles of O₂(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(9) to be 4.35x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = Submit Answer Try Another Version 10 item attempts remaining
The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K.PCl5(g) PCl3(g) + Cl2(g)Calculate the equilibrium concentrations of reactant and products when 0.246 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K. [PCl5] = M [PCl3] = M [Cl2] = M
A student ran the following reaction in the laboratory at 700 K: H2(g) + I2(g) 2HI(g) When she introduced 0.197 moles of H2(g) and 0.231 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of HI(g) to be 0.332 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =