Consider the following reaction at equilibrium. C(6) + 2H,@) = CH,@) + heat How will increasing the pressure on the system affect the amount of each of the substances if the temperature is kept constant? O The amount of reactants will increase and the amount of product will decrease. ) The amount of all substances will increase. ) The amount of product will increase and the amount of reactants will decrease. ) The amount of all substances will decrease. O O

Consider the following reaction at equilibrium. C(6) + 2H,@) = CH,@) + heat How will increasing the pressure on the system affect the amount of each of the substances if the temperature is kept constant? O The amount of reactants will increase and the amount of product will decrease. ) The amount of all substances will increase. ) The amount of product will increase and the amount of reactants will decrease. ) The amount of all substances will decrease. O O

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

Decide whether each of the following statements is true or false. If false, change the wording of the statement to make it true. a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction. d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.
A reaction has a negative ΔH in the forward direction. If the system is initially at equilibrium, what happens to the amount of product if the temperature is lowered?
Which of the following is true for a system whose equilibrium constant is much greater than one? The reaction mixture contains mostly products at equilibrium. The reaction mixture contains mostly reactants at equilibrium. O The rate of reaction is very fast. The moles of reactants and products are relatively similar at equilibrium. Both A and C.
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?
What happens to a system when products are added to a reaction vessel? O The amount of products increases. O The amount of reactants increases. O The amount of reactants decreases. O The system remains at equilibrium.
Consider the reversible reaction. PCI, = PCI, + Cl, What substances are present at equilibrium? PCI, PCI, O Cl, Are the concentrations of phosphorus pentachloride, PCI,, and phosphosphorus trichloride, PCl, , constant or changing at equilibrium? The concentrations of both PCl, and PCl, are changing at equilibrium. The concentration of PCl, is constant, and the concentration of PCl, is changing at equilibrium. The concentration of PCl, is changing, and the concentration of PCl, is constant at equilibrium. The concentrations of both PCl, and PCl, are constant at equilibrium.
thanks you for any help!
The following figure is humorous but it emphasizes an important characteristic of either a chemical or physical equilibrium. What is it? We're back! I'm sure glad they evaporated! Then I'm getting out of here! A) Equilibrium occurs when all processes come to an end. B) Equilibrium is temperature independent. · C) Equilibrium is reached when the number of reactant and product molecules is the same. D) Equilibrium is dynamic. E) Equilibrium depends on where you start the process. rch inort sc delete 8. backspa K pause
For the reaction at equilibrium: 2 H2O (g) +2 Cl2 (g) + energy 4 HCI (g) + O2(g), If a catalyst is added to the reaction mixture. The equilibrium will shift to the left. The equilibrium will shift to the right. The position of the equilibrium will not change.
Phosphorus pentachloride decomposes at higher temperatures. PC15 (8) PCl3(g) + Cl₂(g) An equilibrium mixture at some temperature consists of 5.81 g PCI, 208.23 g/mol 4.86 g PC3, 137.33 g/mol 3.59 g Cl₂, 70.91 g/mol in a 1.00-L flask. If you add 1.31 g of Cl₂, how will the equilibrium be affected and what will the concentration of PCI, be when equilibrium is reestablished? O shift left O shift right Ono shift will occur [PCI5] = mol/L