Antimony(V) chloride, SbCls, dissociates on heating to give antimony(III) chloride, SbCls, and chlorine. SbC15 (9) SbCl3 (g) + Cl₂(g) A closed 3.30 L vessel initially contains 1.39 x 10-2 mol SbCl5. What is the total pressure at 248°C when equilibrium is achieved? The value of Ke at 248°C is 2.50 × 10-2. Pressure = atm

Antimony(V) chloride, SbCls, dissociates on heating to give antimony(III) chloride, SbCls, and chlorine. SbC15 (9) SbCl3 (g) + Cl₂(g) A closed 3.30 L vessel initially contains 1.39 x 10-2 mol SbCl5. What is the total pressure at 248°C when equilibrium is achieved? The value of Ke at 248°C is 2.50 × 10-2. Pressure = atm

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

3. Please provide the correct answer choices for all parts to this chemistry problem.
The equilibrium constant, Ke, for the following reaction is 10.5 at 350. K. 2CH₂Cl₂ (9) CH₂(g) + CCL4 (9) Calculate the equilibrium concentrations of reactant and products when 0.359 moles of CH₂Cl₂ (g) are introduced into a 1.00 L vessel at 350. K [CH₂Cl₂]-[ [CH]-[ [CCL]-[ M M M 3
Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4 (g) + H2O (g) ⇌ H2 (g) + CO (g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations, at a temperature of 760 °C? CH4 = 0.126 M H2O = 0.242 M CO = 0.126 M H2 = 1.15 M Please show Given, Required, Solution. Thank you very much.
The formation of nitrogen monoxide from its elements has an equilibrium which favors reactants: N2 (g) + 02 (g) 2 NO (g) K, = 0.0290 at 2400°C If the initial partíal pressures of both reactant gases are 0.717 atm, what will be the equilibrium partial pressure of nitrogen monoxide? (A certain simplification is valid in solving this problem). 0.112 atm (A) (B) 0.0290 atm (C) 0.688 atm (D) 0.0563 atm (E) 0.0611 atm
Consider the following reaction where K. = 1.29x102 at 600 K. COCl»(g) eCO(g) + Cl2(g) A reaction mixture was found to contain 0.107 moles of COCI,(g), 2.44x102 moles of CO(g), and 4.39×102 moles of Cl2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
A reaction vessel contains an equilibrium mixture of SO2, O2, and SO3. The reaction proceeds such that: 2S0, (g) +0,(g) = 2SO3 (g)
: Given : A (g) +B (g) 2C (g) An equilibrium mixture contains 0,5 mol of each of A and B and 3.5 mol of C in one-liter container at a certain temperature. (a) How many moles of C must be added to the con- tainer to increase the new equilibrium mole number of A to 0.75? (b) If 1 mol of each of A, B and C is added to the first equilibrium mixture, what will be the new equi- librium concentration of each species at the same temperature?
Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5⁢(g)⁢↽−−⇀⁢PCl3⁢(g)+Cl2⁢(g) A 13.1 gsample of PCl5 is added to a sealed 1.25 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 48.4% of the PCl5 remains. What is the equilibrium constant, Kc , for the reaction?
Carbon monoxide and hydrogen react acconding to the following equation: colo) + 3I1, (a) CH.Co) + H,0G) When 1.000 mol CO and 3.000 mol Ha are placed in a 10.00-L. vessel at a high temperature and allowed to come to equilibrium, the mixture is found to contain 0396 mol H0. What is the molar composition of the equilibrium mixture? That is, how many moles of each substance are present mol CO mol H mol CH
Q2
Carbon tetrachloride can be produced by the following reaction: C5₂(g) + 3Cl₂(g) + S₂Cl₂(g) + CCl₂) In an experiment, 0.120 mol of CS₂ and 0.360 mol of Cly were placed in a 1.00-L flask at a particular temperature. After equilibrium has been achieved, the mixture contains 0.040 mol CCl Calculate the value of K under the experimental conditions
The equilibrium constant, Ko, for the following reaction is 10.5 at 350 K: 2CH,Cl2(g)= CH4(g) + CCI4(g) Calculate the equilibrium partial pressures of all species when CH,Cl,(g) is introduced into an evacuated flask at a pressure of 0.606 atm at 350 K. PCH;Cl2 = atm PCHA atm Pccla atm