A student ran the following reaction in the laboratory at 479 K:PCI3(g) + Cl₂(g) =PC15(g)When she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of PCI3 was 2.13 atm and the initial partial pressure of Cl₂ was 1.34 atm, she foundthat the equilibrium partial pressure of PCI5 was 1.12 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction.KpSubmit AnswerRetry Entire Group8 more group attempts remaining

Answered: Image /qna-images/answer/e4c13cf0-d663-4801-8768-2e75dbd24bb0.jpg

udent ran the following reaction in the laboratory at 479 K: (g) + Cl₂(9) ⇒PCI5(9) n she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial the equilibrium partial pressure of PCI5 was 1.12 atm. ulate the equilibrium constant, Kp, she obtained for this reaction. mit Answer Retry Entire Group 8 more group attempts remaining

udent ran the following reaction in the laboratory at 479 K: (g) + Cl₂(9) ⇒PCI5(9) n she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial the equilibrium partial pressure of PCI5 was 1.12 atm. ulate the equilibrium constant, Kp, she obtained for this reaction. mit Answer Retry Entire Group 8 more group attempts remaining

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

None
At 20 °C, the following concentrations were found for the gases in an equilibrium mixture for the reaction N20(g) + NO2(3) 3NO(g) [NO2] = 0.80 M, [NO] = 2.0 x 10°8 M, and [N,0] = 0.034 M. What is the value of K, for this reaction? Enter your answer in scientific notation. Kp : = i x 10 i
Visited 20, E C Use the References to access important values If needed for this question. The equilibrium constant, Ke, for the following reaction is 0.0180 at 698 K. 2HI(g) H₂(g) + 1₂ (9) Calculate the equilibrium concentrations of reactant and products when 0.361 moles of HI(g) are introduced into a 1.00 L vessel at 698 K. [HI] = [H₂] = [1₂] = Submit Answer $ 4 R F FA V M M M % 5 Show Hint Retry Entire Group 9 more group attempts remaining T Cengage Learning Cengage Technical Support F5 G ^ 6 B MacBook Air Y H & 7 U N * 8 M ( 9 ►► K F9 O ) < O A L F10 P 4) - Previous ? { + [ Next = Save and Exit 4) F12 11 (
i need the ans asap
Write the expression for the equilibrium constant K,, for the following reaction. Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH) as (P NH3)² If either the numerator or denominator is 1, please enter 1 3 PbO2(s) Pb304(s) + O2(g) K =
Please help asap!
Part A The reaction N2(g) + O2(9)=2NO(g) is carried out at a temperature at which K = 0.070. The reaction mixture starts with only the product, [NO]=0.0500 M, and no reactants. You may want to reference (Page) Section 15.8 while completing this problem. Find the equilibrium concentrations of N2 at equilibrium. Express your answer to two significant figures and include the approp ΜΑ [N2] = Value Units Submit Request Answer Part B Find the equilibrium concentrations of O2 at equilibrium. Express your answer to two significant figures and include the appropr
The decomposition of HI at low temperature was studied by injecting 2.50 mol of HI into a 10.32-L vessel at 25℃. What is [H2] at equilibrium for the reaction 2HI(g) H2(g) + I2(g); Kc = 1.2610-3 ?
Magnitude of the Equilibrium Constant 7 of 22 Review | Constants | Periodic Ta Part D For a reaction For the reaction aA + bB = cC + dD CO(g) + H2O(g) = H2(g) + CO2(g), K = 4.24 at 800 K the equilibrium constant K is defined as the ratio of products to reactants at equilibrium: what can be said about this reaction at this temperature? K [C]°D]* • View Available Hint(s) [A]*[B]* Because K represents the ratio of products to reactants, the magnitude of K is an indicator of the levels of products and reactants present when the reaction is at equilibrium. Some chemical reactions proceed almost fully to product, whereas other chemicals hardly react with each other at all, or react so as to have significant amounts of both reactants and products at equilibrium. O The equilibrium lies far to the right. O The reaction will proceed very slowly. O The reaction contains significant amounts of products and reactants at equilibrium. O The equilibrium lies far to the left.
35 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 3.01 × 10³ at 900 K. If an initial mixture of 0.0216 mol SO2 and 0.0148 mol O2 reacts in a 1.0 L vessel, what will be the concentration of SO3 at equilibrium? 2 SO:(g) + O2(g)= 2 SO:(g) 1 3 NEXT Based on the given values, set up ICE table in order to determine the unknown. 2 SO:(g) O:(g) + 2 SO:(g) Initial (M) 0.0216 0.0148 Change (M) 0.0216 - 2x 0.0148 - x Equilibrium (M) 5 RESET 0.0216 0.0148 1.0 +x +2x -2x 0.0216 + x 0.0216 + 2x 0.0216 - x 0.0216 - 2x 0.0148 + x 0.0148 + 2x 0.0148 - x 0.0148 - 2x
Please don't provide handwritten solution .....
A student ran the following reaction in the laboratory at 1080 K: 2SO3(g) 2S02(g) + O₂(g) When he introduced SO3(g) at a pressure of 0.886 atm Into a 1.00 L evacuated container, he found the equilibrium partial pressure of SO3(g) to be 0.340 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer 44 $ T R F V/ % 5 Retry Entire Group 9 more group attempts remaining T Cengage Learning Cengage Technical Support F5 G ^ 6 MacBook Air Y H & 7 RN U * 0 J ► 11 F8 M ( 9 ►► K F9 O 1 F11 + { Save and Exit = F12 11