**Equilibrium Constant Calculation**The equilibrium constant \( K_p \) for the reaction:\[ 3A(g) + B(s) \rightleftharpoons C(g) + D(g) \]is \( 4.9 \times 10^{-5} \) at 142°C. What is \( K_c \) for this reaction?Recall that \( K_p = K_c(RT)^{\Delta n} \)Constants:- \( R = 8.31446 \, \text{J} \cdot \text{K}^{-1} \cdot \text{mol}^{-1} \)- \( R = 0.0820573 \, \text{L} \cdot \text{atm} \cdot \text{K}^{-1} \cdot \text{mol}^{-1} \)**Scientific Notation Instruction:**Scientific notation in a canvas quiz is expressed as in the following example:- \( 0.0012 = 1.2 \times 10^{-3} \)Type your answer in the space below.

Calculate the KC value for the given reaction from the given KP value. Given: KP = 4.9×10-5 T…

The equilibrium constant Kp for the reaction 3A(g) + B(s) <--> C(g) + D(g) is 4.9 x 10 5 at 142 °C. What is Kc for this reaction? Recall that Kp =KCRT)An 80 R= 8.31446 J - K-1. mol 1 R= 0.0820573 L atm · K . mol Scientific notation in a canvas quiz is expressed as in the following example: 0.0012 = 1.2*10^-3

The equilibrium constant Kp for the reaction 3A(g) + B(s) <--> C(g) + D(g) is 4.9 x 10 5 at 142 °C. What is Kc for this reaction? Recall that Kp =KCRT)An 80 R= 8.31446 J - K-1. mol 1 R= 0.0820573 L atm · K . mol Scientific notation in a canvas quiz is expressed as in the following example: 0.0012 = 1.2*10^-3

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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1. For the reaction: 2NH3(g) + CO2(g) (NH2)2CO(s) + H2O(g) AH = - 330 kJ Predict how each of the following changes would impact a reaction that is currently at equilibrium. That is, which way would the reaction progress in order to respond to the change in the system to regain equilibrium (use arrows to show the direction of change that would occur to return back to equilibrium). Explain your reasoning for each part.
Consider the following equilibrium: 2NH, (g) – N, (g) + 3H, (g) AG° = 34. kJ Now suppose a reaction vessel is filled with 5.02 atm of ammonia (NH,) and 9.40 atm of nitrogen (N,) at 159. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N, tend to rise or fall? fall Is it possible to reverse this tendency adding H2? In other words, if you said the pressure of N, will tend to rise, can that be yes changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of N, will tend to fall, can that be changed to a tendency to rise by adding H2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, needed to reverse it. atm Round your answer to 2 significant digits.
Nitric oxide reacts with chlorine to form NOCI. 2NO(g) + Cl2g) → 2NOCI(g) The equilibrium constant K at 298K is x 107. (R = 8.314 J/K • mol) Substance: NO(g) Cl2g) NOCIG) AH°F (k]/mol) at 298 K 90.29 51.71 S°U/K• mol) at 298 K 210.65 223.0 261.60
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
3. Phosphoryl chloride, POCI3(g), is used in the manufacturing of flame retardants. It is manufactured in an equilibrium process in which phosphorus trichloride reacts with nitrogen dioxide to form POCI3(8)and NO(g) according to the following equation: PCI3 (g) + NO2 (g) = POCI3 (g) + NO (g) The Keg for this reaction at 800 K is 6.90. If 1.25 mol PCI3 (g) and 1.94 mol NO2 (g) are placed into a 2.0 L container, what is the concentration of each gas at equilibrium at 800 K? PCI3 (g) NO2 (g) POCI3 (g) NO(g) Keq = 6.90 + + E
At 487 K, this reaction has a Ke value of 0.0463. 2 X(g) + 3 Y(g) = 2Z(g) Calculate Kp at 487 K. Note that the pressure is in units of atmosphere (atm). Kp =
Consider the following equilibrium: 2NH3(g) = N₂ (g) + 3H₂(g) 2 AG = 34. kJ Now suppose a reaction vessel is filled with 7.87 atm of ammonia (NH3) and 1.17 atm of hydrogen (H₂) at 448. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise fall yes no atm x10 X 5
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For the following reaction: NH4Cl(s) ↔ NH3(g) + HCl(g) ΔH = +42.1 kilocalories Suppose the substances in the reaction above are at equilibrium at 600K in volume V and at pressure P. State whether the partial pressure of NH3(g) will have increased, decreased, or remained the same when equilibrium is reestablished after each of the following disturbances of the original system. Some solid NH4Cl remains in the flask at all times. Justify each answer with a one-or-two sentence explanation. (e) A quantity of gaseous NH3 is added. The answer for e states that the partial pressure of NH3 is increase, which is a bit confusing. The explanation is that some of the the added NH3 reacts with HCl to relieve stress but only part of NH3 reacts. Can you explain how and where this is implied in the reaction or question. Would appreciate a lot of clarification
Consider the following equilibrium: 2NH3(g) → N₂(g) + 3H₂(g) AG = 34. kJ Now suppose a reaction vessel is filled with 6.39 atm of ammonia (NH3) and 0.200 atm of hydrogen (H₂) at 206. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. OO U rise fall yes no atm x10 X Ś