For the reaction below predict what happened to the temperature for the equilibriums to shift in the scenarios below PCl; (g) + heat = PC13 (g) + Cl2 (g) If the equilibrium shifts to the reactants that means that the temperature If the equilibrium shift to the products that means that the temperature

For the reaction below predict what happened to the temperature for the equilibriums to shift in the scenarios below PCl; (g) + heat = PC13 (g) + Cl2 (g) If the equilibrium shifts to the reactants that means that the temperature If the equilibrium shift to the products that means that the temperature

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

The reaction below was allowed to react at 375 degrees Celcius until it formed an equilibrium. At equilibrium, the 16.2 L container was found to contain 1.9 mol SiF4, 1.1 mol H2O, 3.5 mol SiO2, and 2.9 mol HF. What is the Kc of the reaction at this temperature? SiF4 (g) + 2H2O (g) <--> SiO2 (s) + 4HF(g)
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.
For the following endothermic reaction at equilibrium: H2S(g) H2(g) + 1/8 S8(s) choose the action that will increase the amount of H2S
Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) AH° = -514 kJ Le Châtelier's principle predicts that the production of CO (g) can be maximized by carrying out the reaction
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
The oxidation of ammonia is a reversible exothermic reaction at equilibrium that proceeds as follows: 4 NH3 (g) + 5 O2 (g) ⇋ 4 NO (g) + 6 H2O (g) If the temperature is decrease, what happens to the concentration of H2O?
2C02 2 2C0+0 Consider the reaction above. If pressure was increase on this equilibrium, how would that affect the amounts of reactants? O They would decrease O They would remain the same O They would increase
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
Dry ice (solid carbon dioxide) is placed in a sealed container. It sublimes to produce carbon dioxide gas and reaches equilibrium at a given temperature. If the amount of dry ice in the container is doubled, then _____________. (After choosing the correct answer justify why in your own words why you chose that answer) CO2 (s) = CO2 (g) A)The amount of CO2 (g) would double. B)The amount of CO2 (g) would increase but not double. C)The amount of CO2 (g) would not change. D)The equilibrium amount of CO2 (s) would be less.
Which way would the equilibrium shift if the temperature was decreased for this reaction (AH = -542 kJ)? H₂ (g) + F₂ (g) → 2HF (g) Shift toward reactants Shift toward products Remain the same None of the above