Enter your answer in the provided box.The equilibrium constant for the reactionis 6.8 × 103 at a certain temperature.2SO2(g) + O2(g) = 2SO3(g)If at equilibrium, [SO2] = 0.0611 M and [GE] = 0.07 M, what is the equilibr1.33X

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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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Nitrosyl bromide decomposes according to the equation given below. If 0.640 mole of NOBr is placed in a 1.00 L flask containing no NO or Br2 it is found that at equilibrium there is 0.460 mole of NOBr. What is the value of Kc for this reaction? 2 NOBr (g) → 2 NO (g) + Br2 (g) 1.38 x 10−2 7.26 7.12 x 10−3 3.52 x 10−2 28.4
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 5.96 × 104: H₂(g) + Cl₂(g) →2 HCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 1.8 mol of HCI. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 HCl(g) H₂(g) + Cl₂(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 H₂(g)+2Cl₂(g) 4 HCl(g) ܢܢ There will be very little H₂ and Cl₂. There will be very little HCI. Neither of the above is true. K = 0 K = 0 x10 X 0/3 ? olo 18 Ar BA
Suppose a 500. mL flask is filled with 1.6 mol of H₂ and 0.30 mol of HI. This reaction becomes possible: H₂(g) + 12₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of I2. You can leave out the M symbol for molarity. initial change equilibrium H₂ 0 1₂ x 0 HI 0 X S
Suppose a 500.mL flask is filled with 1.5mol of CO, 1.1mol of H2O and 1.6mol of H2. The following reaction becomes possible: CO(g)+H2O(g)+CO2(g)+H2(g) The equilibrium constant K for this reaction is 0.840 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 1.7 mol of NO2, 0.80 mol of CO and 0.70 mol of CO2. The following reaction becomes possible: NO2(g) + CO(g) = NO(g) + CO2(g) The equilibrium constant K for this reaction is 2.90 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
Which of the following equilibrium expressions (K) represent the equilibrium reaction: 2 Fe(s) + 3 Cl2(g) = 2 FeCl3(s)
Enter your answer in the provided box. The equilibrium constant K. for the equation 2H2(g) + CO(g)=CH3OH(g) is 13 at a certain temperature. If there are 2.21 × 102 moles of H2 and 2.33 x 103 moles of CH;OH at equilibrium in a 4.31-L flask, what is the concentration of CO? M
When 0.16 mol of O2 gas and excess graphite were placed in a 2.00-L container and come to equilibrium, the concentration of CO gas was 0.088 0.024 M. What is the equilibrium constant, Kc, for this reaction at this temperature? Please report 4 decimal places, without units. C(s) + O2(g) ⟷ 2CO(g)
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 NO(g) + Cl₂(g) = 2 NOC1 (g) K₁₂=4.×100 He fills a reaction vessel at this temperature with 8.0 atm of nitrogen monoxide gas and 7.5 atm of chlorine gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NOC1, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NOC1 at right. Round your answer to 1 significant digit. O yes O no 0 atm X
Write the equilibrium-constant expression for the reaction shown in terms of [SO2], [CO2], [CS2], and [O2]. 2SO2(g)+CO2(g)↽−−⇀CS2(g)+3O2(g) ?c, which is sometimes symbolized as ? or ?eq, denotes that the equilibrium constant is expressed using molar concentrations. For this question, ?c means the same thing as ? and ?eq.
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Enter your answer in the provided box. The equilibrium constant for the reaction is 6.8 × 103 at a certain temperature. 2SO2(g) + O2(g) = 2SO3(g) If at equilibrium, [SO2] = 0.0611 M and [GE] = 0.07 M, what is the equilibr 1.33 X