7:40 i 65% on.masteringchemistry.com :D The equilibrium constant, K., is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp = K.(RT)An 0.08206 L · atm/(K· mol), T is the absolute temperature, and An is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction where R N2(g) + 3H2(g) = 2NH3 (g) for which An = 2 – (1+ 3) = -2. Part A For the reaction 3A(g) + 2B(g)= C(g) Kc = 75.8 at a temperature of 75 °C. Calculate the value of Kp. Express your answer numerically. • View Available Hint(s) 7:40 session.masteringchemistry.com/myct/itemView?offset=next&attemptNo=1&ass :D

7:40 i 65% on.masteringchemistry.com :D The equilibrium constant, K., is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp = K.(RT)An 0.08206 L · atm/(K· mol), T is the absolute temperature, and An is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction where R N2(g) + 3H2(g) = 2NH3 (g) for which An = 2 – (1+ 3) = -2. Part A For the reaction 3A(g) + 2B(g)= C(g) Kc = 75.8 at a temperature of 75 °C. Calculate the value of Kp. Express your answer numerically. • View Available Hint(s) 7:40 session.masteringchemistry.com/myct/itemView?offset=next&attemptNo=1&ass :D

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...

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Be sure to answer all parts. The equilibrium constant Ke for the reaction H₂(g) + CO₂(g) = H₂O(g) + CO(g) is 4.2 at 1650°C. Initially 0.75 mol H₂ and 0.75 mol CO₂ are injected into a 4.8-L flask. Calculate the concentration of each species at equilibrium. Equilibrium concentration of H₂: M Equilibrium concentration of CO₂: M Equilibrium concentration of H₂O: M Prex 17 of 27 ‒‒‒ -
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Consider the following gas-phase reaction: 2 NO(g) = N₂(g) + O₂(0) Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG=0) and choose whether A>Gº will increase, decrease, or not change with increasing temperature from the pulldown menu. K. and AG will -Select-- with increasing temperature. For each of the temperatures listed below calculate AG for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ("near equilibrium" means that T is within 5 K of T.). (a) At T-10959 K AG- (b) At T 3653 K AG - (c) At T-7306 K AG- kJ/mol, and the reaction is Select- kl/mol, and the reaction is-Select- kd/mol, and the reaction is-Select- under standard conditions. MY NOTES under standard conditions under standard conditions
uju ts Search G Free Online Survey... Submit Answer Home - Academia... H Modules Retry Entire Group Consider the following reaction where K = 6.50x10-3 at 298 K: 2 NOBr (g) 2 NO(g) + Br₂ (g) A reaction mixture was found to contain 8.48x10-2 moles of NOBr (g), 4.39x10-2 moles of NO (g), and 4.04x10-2 moles of Br₂ (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium NOBr(g) must be consumed. 2. In order to reach equilibrium K must increase. 3. In order to reach equilibrium NO must be produced. 4. Q is less than K. 5. The reaction is at equilibrium. No further reaction will occur. 8 Use the References to access important values. f needed for this question. Create Your Rubric-... [References] K 8 more group attempts remaining 9 The Utility Experts ... PPT 4:33 PM 12/15/2023 prt sc backspace
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Consider the reaction of N₂O and O2 described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. NEXT > A 1.00 L reaction vessel was filled with 0.0560 mol O₂ and 0.200 mol N₂O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) 0.0100 0.0410 0 -0.0100 0.0710 1 2 N₂O(g) + 3 O₂(g) = 4 NO2(g) 2N₂O(g) 0.0560 -0.0050 0.0360 0.200 0.0050 0.180 + -1.00 0.0150 30₂(g) 2 -0.0560 -0.0150 0.0200 0.210 4NO₂(g) RESET -0.0200 0.190 +
The equilibrium constant, Kp, for the following reaction is 1.80x102 at 698 K: 2HI(g) = H₂(9) + I₂(9) Calculate the equilibrium partial pressures of all species when HI(g) is introduced into an evacuated flask at a pressure of 1.23 atm at 698 K. PHI= PH₂= 4 P1₂ = $ Submit Answer 900 F4 R F T V % 5 atm atm atm T Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support F5 G ^ 6 B MacBook Air Y H & 7 N F7 U J * 8 ► 11 - M -a 9 K >> ded for this question. F9 O 4) Previous Next> F11 Save and Exit 4) F12 11 I C
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)