For the following "possible" reaction, which are the states of the products in order from left to right. C 3CaS (aq) + Al₂(SO4)3 (aq) 3CaSO4( ) + Al2S3 ( ) CATIONS Os, s High Solubility (aq) Low Solubility (s) aq, s s, aq OI,I aq, aq Cl, Br, I Halides Most Ag+, Pb²+, Tl+, Hg₂²+, Hg', Cu S2- Solubility Table Group 1, Nhì, Group 2 Most ANIONS OH Group 1, NH4*, Sr²*, Ba²+, Tl Most SO4²- Most Ag+, Pb²+, Ca²+, Ba²+, Sr²., Ra² CO3²-, C₂H30₂ NO3 PO4³, SO3²- All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. Group 1, NH Most Most All Ag+ None

For the following "possible" reaction, which are the states of the products in order from left to right. C 3CaS (aq) + Al₂(SO4)3 (aq) 3CaSO4( ) + Al2S3 ( ) CATIONS Os, s High Solubility (aq) Low Solubility (s) aq, s s, aq OI,I aq, aq Cl, Br, I Halides Most Ag+, Pb²+, Tl+, Hg₂²+, Hg', Cu S2- Solubility Table Group 1, Nhì, Group 2 Most ANIONS OH Group 1, NH4, Sr², Ba²+, Tl Most SO4²- Most Ag+, Pb²+, Ca²+, Ba²+, Sr²., Ra² CO3²-, C₂H30₂ NO3 PO4³, SO3²- All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. Group 1, NH Most Most All Ag+ None

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

What will happen if the system is cooled? What will happen if more CO2 (g) is added?
The reaction quotient (Q) for a system is 70. If Kc = 35, what will happen as equilibrium is approached? Othere will be a net gain in product the reaction is at equilibrium O there will be no net gain in either product or reactant. there will be a net gain in reactant there will be a net gain in both reactant and product
Chemistry
For the following equilibrium reaction: 2NO2(g) N2O4(g) + Δ What happens if the volume of the reaction is decreased?
A sample of solid potassium nitrate is placed in water. The solid potassium nitrate comes to equilibrium with its dissolved ions by the endothermic process shown below. KNO₂ (s) + energy →K*(aq) and NO₂ (aq) Which of the following changes to the system would increase the concentration of K* ions at equilibrium? (A) The volume of the solution is increased (B) The volume of the solution is decreased (C) Additional solid KNO3 is added to the solution (D) The temperature of the solution is increased
The equilibrium constant for the following equilibrium reaction is: 2Hg (l) + O2 (g) 2HgO (s)
30. The following reaction takes place. A,B(s) = 2A(ac) + B(ag) + heat. If 1.80 moles of A,B is added into a 1.00 L container, it is found that 30.0% of the reactant dissociates to reach equilibrium. Find the solubility product constant, Ksp, for this reaction. Note: Your answer must include an ICE table. (aq),
Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. The equilibrium will not shift The equilibrium will shift toward product but Keq will not change The equilibrium will shift toward reactant but Keq will not change The equilibrium will shift toward product but Keq will will increase The equilibrium will shift toward reactant but Keq will decrease(b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%.
Ff.294.
For the reaction 2 NO2 (g) <-=> N2O4 (g) , Kp =_____ Kc(RT) Kc/RT (RT)/Kc Kc
Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron/iron oxide catalyst. For the reaction: N₂(g) + 3H₂(g) → 2NH3(g) AH -92.22 kJ/mol At 300 °C the equilibrium constant for the reaction is 4.34 x 10-³. a) Is this reaction endothermic or exothermic? b) What effect would the following changes have on the equilibrium position. Write forward, reverse or no change: • Add some more nitrogen gas • Increase the volume of the reaction vessel • Decrease the temperature • Remove some hydrogen gas
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