At -9.93 °C the concentration equilibrium constant K = 6.2 for a certain reaction.Here are some facts about the reaction:• Some of the reactants are liquids and solids.-1• The initial rate of the reaction is 7.9 mol·L¹.s¹..If the reaction is run at constant pressure, the volume increases by 9.5%.Yes.☐ x10Using these facts, can you calculate K, at -29. °C?5No.If you said yes, then enter your answer at right. Round it to2 significant digits.If you said no, can you at least decide whether K at-29. °C will be bigger or smaller than K at -9.93 °C?Yes, and K will bebigger.Yes, and K will besmaller.No.

The objective of the question is to answer the questions related to the information provided by the…

At-9.93 °C the concentration equilibrium constant K = 6.2 for a certain reaction. Here are some facts about the reaction: • Some of the reactants are liquids and solids. • The initial rate of the reaction is 7.9 mol-L-1 -1 . .If the reaction is run at constant pressure, the volume increases by 9.5%. ○ Yes. Using these facts, can you calculate K at -29. °C? O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. 0] at If you said no, can you at least decide whether K -29. °C will be bigger or smaller than K, at -9.93 °C? Yes, and K will be bigger. Yes, and K will be smaller. No. X G

At-9.93 °C the concentration equilibrium constant K = 6.2 for a certain reaction. Here are some facts about the reaction: • Some of the reactants are liquids and solids. • The initial rate of the reaction is 7.9 mol-L-1 -1 . .If the reaction is run at constant pressure, the volume increases by 9.5%. ○ Yes. Using these facts, can you calculate K at -29. °C? O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. 0] at If you said no, can you at least decide whether K -29. °C will be bigger or smaller than K, at -9.93 °C? Yes, and K will be bigger. Yes, and K will be smaller. No. X G

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

At -14.3 °C the concentration equilibrium constant K =5.5 x 10 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, 85.0 kJ/mol of heat are released. • Some of the reactants are liquids and solids. • If the reaction is run at constant pressure, the volume increases by 10.%. OYes. Using these facts, can you calculate K at 1.5 °C? O No. X. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K will be bigger. If you said no, can you at least decide whether K at Yes, and K will be 1.5 °C will be bigger or smaller than K at -14.3 °C? smaller.
Consider the following equilibrium with K = 2.3 x 10-6: N2 ) + 3H2 (g) 2NH3 (g) 0.1 moles of N2, 0.1 moles of H2, and 0.01 moles of NH3 are placed in a 1 L container. Which of the following is true? O Q > K, the reaction will produce more products O Q = K, the reaction is at equilibrium O Q K, the reaction will produce more reactants
A chem gineer is studying the following reaclon! HCN(aq)+NH,(aq) - CN (aq)+NH,(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.99. The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel compound concentration expected change in concentration HCN 0.84 M O t increase OI decrease O (no change) NH, 1.00 M O t increase O, decrease O (no change) CN 0.42 M O 1 increase O. decrease O (no change) NH, 0.33 M O t increase O, decrease O (no change) HCN 1.01 M O t increase O. decrease O (no change) NH, 1.17 M O t increase O. decrease O (no change) CN 0.25 NM M t increase O. decrease O (no change) NH. 0.16 MM O t increase O.…
5. The equilibrium constant expression of a gas reaction is [CS2] [H2]* _ [CH4] [H2S]? K. Write the balanced chemical equation corresponding to this expression
In air at 25 °C and 1.00 atm, the N₂ concentration is is 0.033 M. The 0.01 M and the O₂ concentration reaction N₂(g) + O₂(g) → 2NO(g) has Kc = 4.8 x 10-31 at 25 °C. C Taking the N₂ and O2 concentrations given above as initial values, calculate the equilibrium NO concentration that should exist in our atmosphere from this reaction at 32 °C, Kc = 2.6E-30. Make simplifying assumptions in your calculations. (Express your answer in scientific notation.) [NO] = i M !
Methanol can be synthesized by combining carbon monoxide and hydrogen. AH Cog) + 2H2(g) CH3OH(g) A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperatu IXn=-90.71J 45°C? OA. All the partial pressures will decrease. OB. The partial pressure of carbon monoxide will decrease. OC. The partial pressure of methanol will decrease. OD. The partial pressures of hydrogen and methanol will decrease. O E. The partial pressure of hydrogen will increase.
Q2
1. Consider the following reaction at 500 K: 2 NO (g) + O2 (g) 2 2 NO2 (g); Kc = 6.9 x 105 This reaction is allowed to reach equilibrium, and then analyzed and found to contain the following concentrations: [O2] = 1.0 x 10-3 M [NO2] = 5.0 x 10-2 M. Determine the equilibrium concentration of NO (g).
Consider the reaction A + B C+D, which has an equilibrium constant, K, equal to 3.4 x 102. If one begins a reaction by placing 0.600 moles of A in a 1.0 L container as well as 0.150 moles of 1. B, what will be the equilibrium concentrations of A, B, C, and D? Write your answers in the spaces provided below. a. [А] b. [B]= [C]= С. d. [D]= Once the reaction in problem 1 reaches equilibrium, some additional B is injected into the flask 2. from an outside source. LeChatelier's principle says the reaction will (circle one): be unchanged shift to the right shift to the left Pyridine is a weak base with a Kb 1.7 x 109. If 0.300 moles of pyridine is added to 1.00 L of 3. water, what will be the equilibrium concentrations of the species below: a. [Pyridine] = b. [Pyridine-H] (the pyridinium ion) [ОН-] 3 С. What is the pH of the solution in problem 4 (above)? .
Answer the question
Consider the reaction shown below at a certain temperature. 2 H20(g) 2 2 H2(g)+ O2(g) The equilibrium constant, K, is equal to 8.7×10' at a certain temperature. At equilibrium, it is found that [H,] =7.9×10-² M and [O2] = 4.1×10-2 M. What is the concentration of H,0 at equilibrium? [H2O] = M
41. Given this reaction at equilibrium: 2C0(g) + 02(g)= 2C02(g). Which statement regarding the reaction is always true? * a. the rates of the forward and reverse reactions are equal O b. the reaction occurs in an open system O c. the masses of the reactants and the products are equal O d. the concentrations of the reactants and the products are equal 42. Which factors must be equal in a reversible chemical reaction at equilibrium? * a. the concentrations of the reactants and products O b. the potential energies of the reactants and products c. the activation energies of the forward and reverse reactions Od. the rates of reaction of the forward and reverse reactions