Kt (for endothermiç)↑ temperature result in ↑product formation in theequilibriumbecause theFavour theIncrease T (Theat) endothermic reactionheat + A=B(for exothermic)mixtureofforward reaction is a fewtimes higher than the rateof backward reactionrateFavour the exothermic K (for endothermic)reactionA=B+ heatDecrease T (theat)Kt (for exothermic)17Question:For a specific reaction, which of the following statements is TRUE about K, the equilibriumconstant?It always remains the same at different reaction conditions.It increases if the concentration of one of the products is increased.It changes with changes in the temperature.It increases if pressure is increased.ABCD

The equilibrium constant (K) is the value that is obtained when the reaction attains equilibrium. It…

↑ temperature result in ↑ product formation in the equilibrium because the rate of forward reaction is a few times higher than the rate of backward reaction Favour the Kt (for endothermic) Increase T (Theat) endothermic reaction KI (for exothermic) heat + A=B mixture Favour the exothermic K (for endothermic) Decrease T (theat) reaction KT (for exothermic) A=B+ heat Question: For a specific reaction, which of the following statements is TRUE about K, the equilibrium 17 constant? It always remains the same at different reaction conditions. It increases if the concentration of one of the products is increased. It changes with changes in the temperature. A B It increases if pressure is increased.

↑ temperature result in ↑ product formation in the equilibrium because the rate of forward reaction is a few times higher than the rate of backward reaction Favour the Kt (for endothermic) Increase T (Theat) endothermic reaction KI (for exothermic) heat + A=B mixture Favour the exothermic K (for endothermic) Decrease T (theat) reaction KT (for exothermic) A=B+ heat Question: For a specific reaction, which of the following statements is TRUE about K, the equilibrium 17 constant? It always remains the same at different reaction conditions. It increases if the concentration of one of the products is increased. It changes with changes in the temperature. A B It increases if pressure is increased.

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

Consider the reaction: N₂O4 (9) 2NO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: N2(g) + 202 (9) ⇒N₂O4(9) K₁ 1/2N₂(g) + O₂(g) NO₂ (g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K
Consider the following system at equilibrium: P4 (g) + 6 H2 (g) = 4 PH3 (g) ΔΗ 110. 5 kJ If the volume was increased, what changes would have to occur to reestablish equilibrium? Select 2 correct answer(s) The reaction would shift right. The concentration of PH3 would increase. The concentration of P4 would increase The reaction would shift left. The concentration of H2 would decrease.
Based on a Kc value of 0.170 and the data table given, what are the equilibrium conversations of XY, X, and Y, respectively?
Given the chemical reaction (R1) below, calculate the numerical value of the equilibrium constant for reaction R2 (give your answer to three sig figs) (R1) 2 NO(g) + O2(g) = 2 NO2(g); Kc = 1.62 (R2) 6 NO(g) + 3 O2(g) = 6 NO2(g)
For the folllowing endothermic reaction at equilibrium: Fe2O3(s) + 3H2 = 2 Fe(s) + 3H2O Decide if each of the following changes will increase the value of K (T=temperature)
The equilibrium constant, Kc, for the following reaction is 1.25 at 659 K. 2NH3 (9) N2(g) + 3H₂(g) When a sufficiently large sample of NH3(g) is introduced into an evacuated vessel at 659 K, the equilibrium concentration of H₂(g) is found to be 0.609 M. Calculate the concentration of NH3 in the equilibrium mixture. [NH3] = Submit Answer Use the References to access important values if needed for this question. M Submit Answer Retry Entire Group 8 more group attempts remaining [Review Topics] [References] Use the References to access important values if needed for this question A student ran the following reaction in the laboratory at 679 K: H₂(g) + I₂(g) → 2HI(g) When she introduced 0.208 moles of H₂(g) and 0.237 moles of I2 (g) into a 1.00 liter container, she found the equilibrium concentration of I2 (g) to be 0.0625 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = | Retry Entire Group 8 more group attempts remaining'
At a certain temperature, the equilibrium constant K for the following reaction is 734.: NO3(g) + NO(g) 2 NO₂(g) Use this information to complete the following table. ?
Quèstion 14 The reaction below is an example of a equilibrium. PCI 5( s) = PCI 3( )+ Cl 2(g) O catalytic O irreversible O polar O homogeneous O heterogeneous A Moving to another question will save this response. SAMSUNG Ce & 4 8. 6. e y
9) Given the following equilibrium reaction below, indicate which direction the reaction will shift when the indicated stresses are applied (à, ß, or none), AND indicate how the K value will change (increase, decrease or stays same) with the stress. P = 1 atm, unless otherwise specified. CO(g) + Cl2(g) ó COCl2(g) H = –107.6 kJ/mol What will happen if:ShiftK value i) The pressure is quadrupled________________________ ii) The reaction temperature is decreased_________________________ iii) More COCl2 gas is added_________________________ iv) The volume is doubled_________________________
Dinitrogen tetroxide partially decomposes according to the following equilibrium: N204(g) = 2NO2(g) A 1.000-L flask is charged with 0.0300 mol of N204. At equilibrium, 0.0204 mol of N204 remains. Calculate the Kc for this reaction. (Enter only the numerical value to three significant figures without units.) Answer:
Select all of the correct statements about equilibrium from the choices below. At equilibrium the rates of forward and reverse reactions are equal. At equilibrium the speed of a reaction equals its rate constant. At equilibrium concentrations of reactants and products stay constant. At equilibrium the reverse rate equals zero. ☐ At equilibrium the rate of change of product concentration is zero. As a reaction proceeds backwards toward equilibrium the product concentrations drop.
all the drop down are right or left