A chemist studying reactions of phosphorus halides. The chemist determinedconcentrations of every substance in the reaction at a certain point as follows:10.1 M of PC15 with 0.18 M of Cl2 and 0.18 M of PC13 at 250 °C.PCI:(g) PCI3(g) + Cl½(g) Ke = 4.2 × 10-2In which direction the reaction proceeds to reach equilibrium?Show your work in details.

Given, The given chemical reaction is follows,PCl5(g)⇌PCl3(g)+Cl2(g) ;Kc =4.2×10-2 [PCl5]…

A chemist studying reactions of phosphorus halides. The chemist determined concentrations of every substance in the reaction at a certain point as follows: 10.1 M of PCI5 with 0.18 M of Cl2 and 0.18 M of PC13 at 250 °C. PCI5(g) PCI3(g) + Cl2(g) K. = 4.2 × 10² In which direction the reaction proceeds to reach equilibrium?

A chemist studying reactions of phosphorus halides. The chemist determined concentrations of every substance in the reaction at a certain point as follows: 10.1 M of PCI5 with 0.18 M of Cl2 and 0.18 M of PC13 at 250 °C. PCI5(g) PCI3(g) + Cl2(g) K. = 4.2 × 10² In which direction the reaction proceeds to reach equilibrium?

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

Phosphorus pentachloride decomposes according to the chemical equation PC15(g) PC13(g) + Cl₂(g) Kc = 1.80 at 250 °C A 0.1584 mol sample of PC1, (g) is injected into an empty 2.00 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PC13 (g) at equilibrium.
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
Explain step by step
The first step in the industrial synthesis of hydrogen is the reaction of steam and methane to give carbon monoxide and hydrogen at 1400 K. H2O(g) + CH4(g) ⇋ CO(g) + 3H2(g) The equilibrium constant, K, is equal to 4.7 at 1400 K. A mixture of reactants and products at 1400 K contains 0.035 M H2O, 0.050 M CH4. 0.15 M CO, and 0.20 M H2. (a) Is this reaction at equilibrium? Hint: how does your calculated ratio of products to reactants compare to the equilibrium constant noted above. (b) In which direction does the reaction proceed to reach equilibrium?
Calculate the equilibrium partial pressure of CO2.
The equilibrium constant, Kc, for the following reaction is 0.00650 at 298 K. 2NOBr(g) ⇒ 2NO(g) + Br₂ (g) If an equilibrium mixture of the three gases in a 15.6 L container at 298 K contains 0.201 mol of NOBr(g) and 0.284 mol of NO, the equilibrium concentration of Br₂ is | M.
N2(g) and O2(g) can exist in equilibrium with NO(g), as shown below. The equilibrium constant at 25.0°C is 4.8 x 10-31. If initially there are 1.35 mol of nitrogen and 0.60 mol of oxygen in a 2.00 L vessel, find the equilibrium concentrations of each species. N2(g) + O2(g) → 2NO(g)
The equilibrium constant, K, for the following reaction is 9.52×10 2 at 350 K. CH, (g) + CCI, (g)=2 CH,Cl, (g) Calculate the equilibrium concentrations of reactants and product when 0.310 moles of CH, and 0.310 moles of CCI, are introduced into a 1.00 L vessel at 350 K. [CH ] M [CCL] =D M [CH,Cl, ] = M
A chemical engineer is studying the following reaction: BF3(aq) + NH3(aq) → BF3NH₂(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.9. с The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B с compound BF 3 NH3 BF₂NH₂ BE 3 NH3 BF, NH3 BF3 NH3 BF3NH₂ concentration 0.65 M 0.70 M 0.88 M 0.03 M 0.07 M 1.06 M 0.04 M 0.08 M 1.05 M expected change in concentration ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↓ decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease ↓ decrease decrease ↓ decrease X (no change) (no change) (no change) (no change) (no change)…
Nitric oxide, NO, reacts readily with chlorine gas as follows: 2NO(+ Cl2(g) 2NOCI(g) At 700 K, the equilibrium constant, K, for the reaction is 0.26. Are the following mixtures of NO, Cl₂ and NOCI at equilibrium? If not, predict the direction in which the reaction will proceed. [NOCI] = 0.11 M a.) [NO] = 0.15 M b.) [NO] = 0.15 M c.) [NO] = 0.12 Man [Cl₂] = 0.31 M, [Cl₂] = 0.20 M [Cl₂] = 0.10 M [NOCU] = 0.051 M I [NOCU] = 0.050 M
2 A reaction quotient, Q, is calculated to be 3.2 x 10. The equilibrium constant for the same reaction is 5.4 x 10³. Which statement is correct? a The system is at equilibrium. b The concentrations of the products are greater than their concentrations at equilibrium. The system will attain equilibrium by moving to the right. The system will attain equilibrium by moving to the left. More information is needed to determine which statement is correct. C d e
At 773 °C, a mixture of CO(g), H2(g), and CH3OH(g) was allowed to come to equilibrium. The concentrations were determined to be: [CO] = 0.105 M, [H2] = 0.250 M, [CH3OH] = 0.00261 M. Calculate K. for the reaction CO(g) + 2H2(g) CH3OH(g) Kc = %3D