Phosphorus pentachloride decomposes at higher temperatures. PC15(g) → PC13(g) + Cl2(g) (a) An equilibrium mixture at some temperature consists of 3.120 g of PC15, 3.845 g of PC13, and 1.787 g of Cl₂ in a 1.00-L flask. If you add 1.418 g of Cl₂, how will the equilibrium be affected? (b) What will the concentrations of PC15, PC13, and Cl₂ be when equilibrium is reestablished? I

Phosphorus pentachloride decomposes at higher temperatures. PC15(g) → PC13(g) + Cl2(g) (a) An equilibrium mixture at some temperature consists of 3.120 g of PC15, 3.845 g of PC13, and 1.787 g of Cl₂ in a 1.00-L flask. If you add 1.418 g of Cl₂, how will the equilibrium be affected? (b) What will the concentrations of PC15, PC13, and Cl₂ be when equilibrium is reestablished? I

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

Carbon dioxide and water react to form methanol and oxygen, like this: 2 CO,(g)+4 H,O(g)→2 CH;OH(1)+3 O,(g) At a certain temperature, a chemist finds that a 4.6 L reaction vessel containing a mixture of carbon dioxide, water, methanol, and oxygen at equilibrium has the following composition: compound amount CO2 3.94 g H,0 4.50 g CH,OH 3.68 g O2 2.67 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. M K = 0 Lo B Cisc M Explanation Check A Chem 02022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility 9 Type here to search (99+ IA ASUS ZenBook Esc F2 F3 F4 F5 F6 F7 F8 %23 %24 21 4. * 6. L. R Y 3)
Q3. At 298 K, F3SSF(g) decomposes partially to SF2(g). At equilibrium, the partial pressure of SF2(g) is 1.1X10-4 atm and the partial pressure of F3SSF is 0.0484 atm. (a) Write a balanced equilibrium equation to represent this reaction. (b) Compute the equilibrium constant corresponding to the equation you wrote. (c) Some SF2 (at a partial pressure of 2.3X10-4 atm) is placed in a closed container at 298 K with some F3SSF (at a partial pressure of 0.0484 atm). Enough argon is added to raise the total pressure to 1.000 atm. Calculate the initial reaction quotient for the decomposition of F3SSF to SF2.
The formation of nitrogen monoxide from its elements has an equilibrium which favors reactants: N2 (g) + 02 (g) 2 NO (g) K, = 0.0290 at 2400°C If the initial partíal pressures of both reactant gases are 0.717 atm, what will be the equilibrium partial pressure of nitrogen monoxide? (A certain simplification is valid in solving this problem). 0.112 atm (A) (B) 0.0290 atm (C) 0.688 atm (D) 0.0563 atm (E) 0.0611 atm
Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s)+3 H,0(g)→ Fe,O3(s)+3 H,(g) At a certain temperature, a chemist finds that a 9.2 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound amount ol. Fe 4.85 g Ar H,O 1.44 g Fe,O3 2.98 g H2 2.51 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 Ox10 Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)–→2 HgO(s) At a certain temperature, a chemist finds that a 6.3 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 5.8 g O2 22.5 g HgO 18.9 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0
At a certain temperature, the equilibrium constant K for the following reaction is 0.0087: NO₂(g) + CO(g) → NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 29. L reaction vessel is filled with 0.27 mol of NO₂ and 0.27 mol of CO. 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 2 significant digits. NO(g) + CO₂(g) NO₂(g) +CO(g) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(g)+2CO(g) 2NO(g)+2CO₂(g) There will be very little NO₂ and Co. There will be very little NO and CO₂. Neither of the above is true. K = 0 0 0 x10 X ?
An equilibrium mixture contains 0.700 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H₂O(g) ⇒ CO₂(g) + H₂(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? moles of CO₂ I mol
Coal can be used to generate hydrogen gas (a potential fuel) by the following endothemic reaction (heat is on the reactant side of the equation). C (3) + H20 (g) = co (g) + H2 (g) If this reaction mixture is at equilibrium, predict whether each of the following will resuit in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. Part A adding more C to the reaction mixture the formation of additional hydrogen gas the formation of less hydrogen gas O no effect on the quantity of hydrogen gas
Nitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no change
When heated, carbon monoxide reacts with water to produce carbon dioxide and hydrogen. CO(g) + H2O(g) <--> CO2(g) + H2(g) +heat For each of the following changes at equilibrium, indicate whether the equilbrium shifts in the directions of the products, the reactants, or does not change: (a) decreasing the temperature (b) adding more H2(g) (c) removing some CO2(g) (d) adding more H2O(g) (e) decreasing the volume of the container
At a certain temperature, the equilibrium constant k for the following reaction is 6.3 x 10*: NO,(g) + CO(g) = NO(g) + CO,(g) Use this information to complete the following table. Suppose a 40. L reaction vessel is filled with 1.1 mol of NO2 and 1.1 mol of Co. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little NO2 and CO. There will be very little NO and CO2. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = NO(9)+CO2(9) NO2(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = | 3 NO,(9)+3CO(9) 3 NO(9)+3CO2(9)
7. Suppose for a synthesis of hydrogen fluoride from hydrogen and fluorine, 3.000 moles of H2 and 6.000 moles of F2 are mixed in a 3.000-L flask. Assume that the equilibrium constant for the synthesis reaction at this temperature is 1.15x102. H2 (g) + F2 (g) ↔ 2HF (g) What is the molar concentration of HF at equilibrium? What is the molar concentration of F2 at equilibrium? At a Kc of 4.15x103, predict the direction of the reaction if the starting concentrations are [H2]=2.30 M, [F2]= 1.25x10-3 M, and [HF]= 4.37 M