Consider the gas phase reaction 2 C(g) = A(g) + B(g) . Experiments show that at pressure 1.0 atm and temperature T = 450 K (Pc/p®)² (Pa/pº) (PB/p°) Кр 1.32 x 10-3 . Notice that at such low pressure the equilibrium gas mixture behaves as an ideal gas mixture. a) What is the value of the equilibrium constant K(T) at the indicated T and p? b) What is the degree of dissociation a number of moles of C dissociated at equilibrium a = initial number of moles C at the indicated T and p when the reaction is started with n moles of C in the absence of the products? Hint: Please notice that a reasonable first step when solving for x an equation of the form A f(x) /g(x)² , (where A is a positive constant and f(x) and g(x) polynomials in x) is to take the square root on both sides of the equation to get the simpler resuly A = f(x)/g(x), and proceed from there.

Consider the gas phase reaction 2 C(g) = A(g) + B(g) . Experiments show that at pressure 1.0 atm and temperature T = 450 K (Pc/p®)² (Pa/pº) (PB/p°) Кр 1.32 x 10-3 . Notice that at such low pressure the equilibrium gas mixture behaves as an ideal gas mixture. a) What is the value of the equilibrium constant K(T) at the indicated T and p? b) What is the degree of dissociation a number of moles of C dissociated at equilibrium a = initial number of moles C at the indicated T and p when the reaction is started with n moles of C in the absence of the products? Hint: Please notice that a reasonable first step when solving for x an equation of the form A f(x) /g(x)² , (where A is a positive constant and f(x) and g(x) polynomials in x) is to take the square root on both sides of the equation to get the simpler resuly A = f(x)/g(x), and proceed from there.

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

I need the answer as soon as possible
For the reaction 3H2(g)+N2(g)⇌2NH3(g) at 225 ∘C the equilibrium contant is 1.7×10 ^2. If the equilibrium mixture contains 0.19 M H2 and 0.015 M N2, what is the molar concentration of NH3? Express your answer to two significant figures and include the appropriate units.
Balance each reaction and write its reaction quotient, Q꜀:
Nitrogen and hydrogen react to form ammonia, like this: N2 (g)+3H,(g) 2NH;(g) Suppose a mixture of N,, H, and NH, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. alo perturbation change in composition shift in equilibrium Ar to the right The pressure of N, will to the left Some H, is removed. The pressure of NH, will (none) to the right The pressure of N, will ? to the left Some NH, is added. The pressure of H, will v ? O (none) go up. go down. not change.
13) Consider the reaction between nitrogen and steam: 2N₂(g) + 6H₂0(g) ⇒ 4NH3(g) + 30₂(g) At a certain temperature, K = 28.6. Calculate the equilibrium partial pressure of steam if PNH₂ = 1.75 atm, Po₂ = 0.963 atm, and P№₂ = 0.996atm at equilibrium.
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if Kc and Qc are within 5% of each other.) (a) 2 NH3(g) equalibrium arrow N2(g) + 3 H2(g), [NH3]i = 0.400 M, [N2]i = 0.155 M, [H2]i = 0.110 M, Kc = 16 What is the reaction quotient? What direction will the reaction shift to? (b) 2 NH3(g) equalibrium arrow N2(g) + 3 H2(g), Pi(NH3) = 2.10 atm, Pi(N2) = 10.70 atm, Pi(H2) = 10.70 atm, Kp = 8.3 ✕ 104 What is the reaction quotient? What direction will the reaction shift to? (c) 2 SO3(g) equalibrium arrow 2 SO2(g) + O2(g), [SO3]i = 1.90 M, [SO2]i = 1.90 M, [O2]i = 1.90 M, Kc = 0.23 What is the reaction quotient? What direction will the reaction shift to? (d) 2 SO3(g) equalibrium arrow 2 SO2(g) + O2(g), Pi(SO3) = 0.100 atm, Pi(SO2) =…
The equilibrium constant, Kc, for the following reaction is 1.29x10-2 at 600 K. coCI,(g) ? CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.373 moles of COCI2(g) are introduced into a 1.00 L vessel at 600 K. [COCI2] = [CO] M [Cl2] M ΣΣΣ
Consider the hypothetical reaction A(g) 2B(g). A flask is charged with 0.74 atm of pure A. after which it is allowed to reach equilibrium at 0 °C. At equilibrium the partial pressure of A is 0.37 atm Part A What is the total pressure in the flask at equilibrium? Express your answer using two significant figures. VS ΑΣΦ 4 P₁ = Submit Part B What is the value of Kp? Express your answer using two significant figures. K₂= Submit Part C Request Answer |VL ΑΣΦ Submit Request Answer What could we do to maximize the yield of B? → Request Answer [w] ? O Doing the reaction in a larger flask maximizes the yield of B. O Doing the reaction in a smaller flask maximizes the yield of B. atm
A reaction vessel at 408.5 K contains a mixture of Cl(g) (P = 3.060 bar) and SO2(g) (P = 1.258 bar). The following reaction occurs: Part A Cl2(g) + SO2(g) SO2CI2(g) Determine the equilibrium constant, K. At equilibrium the total pressure is 3.126 bar.
For the reaction X(g)+3Y(g)⇌3Z(g) Kp = 1.95\times 10−2 at a temperature of 81 ∘C . Calculate the value of Kc .
The equilibrium constant for the chemical equation N2(g)+3H2(g)↽−−⇀2NH3(g) N 2 ⁡ ( g ) + 3 ⁢ H 2 ⁡ ( g ) ⁢ ↽ − − ⇀ ⁢ 2 ⁢ NH3(g) is Kp = 0.249 at 253 ∘C. 253 ⁢∘ C. Calculate the value of Kc for the reaction at 253 ∘C
Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) K = 4.3 x 10-25 2NO(g) + O2(g) == 2NO,(g) K= 6.4 × 10' Determine the value of the equilibrium constant for the following equation at the same temperature: N2(g) + 202(g) = 2NO2(g) K. - x 10 (Enter your answer in scientific notation.)