Adding reactant will shift reaction toward right.
Adding product will shift reactiom toward left.
1)a) Adding H2O will shift reaction toward left.
b) NH3 will react with Ag+ to form a complex [Ag(nh3)2]+
So, the reaction will shift toward left.
c) KI will react with Ag+ to form AgI precipitate. So,reaction will shift toward left.
d) Adding carbon will shift reaction toward right.
e) catalyst do not affect the reaction equillibrium.
. Predict the direction of the equilibrium for the following reaction by stating left, right, or...
Indicate the direction( left or right) of equilibrium shift when the acompanying stress is applied to the system: HCL (aq) is added to 4CL- (aq) + Co(H2O)62+ = CoCL42- (aq) + 6H2O(l) ****please address how the common-ion effect is observed in this reaction and how it influences the equilibrium****
For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase NH3(g)+H2O(l) ⇋ NH4+(aq)+OH−(aq) Drag the appropriate stresses to their respective bins. Adding NH4+(aq) Adding NH3(g) Adding OH-(aq) Removing NH4+(aq) Removing OH-(aq) Shifts in the direction of the reactants: Shift in the direction of the products:
1. Which of the following reaction represents cathode reaction in chrom plating? a. Cr (s) → Cr6+ (aq) + 6 e¯ b. Cr (s) → Cr3+ (aq) + 3 e¯ c. Cr3+ (aq) + 3 e¯ → Cr (s) d. Cr (s) → Cr3+ (aq) + 6 e¯ 2. The molar solubility of AgBr is 6.3 × 10−7 M. What is its Ksp? 3. Co2+ (aq) + 6 H2O (l) ⇌ Co(H2O)62+ (aq) the ligand(s) is/are: a. Co2+ b. Co(H2O)62+...
4.) (20%) Which one of the following is an acid base reaction? a) C(s) + O2(g) → CO2(g) b) 2 HCl(aq) + Ca(OH)2(aq) + 2 H2O(1) + CaCl2(aq) c) Fe(s) + 2 AgNO3(aq) — 2 Ag(s) + Fe(NO3)2(aq) d) MgSO4(aq) + Ba(NO3)2(aq) + Mg(NO3)2(aq) + BaSO4(s) e) None of the above are acid base reactions.
Consider the following equilibrium reaction: 4NH3(g) + 5O2(g) <---> 4NO(g) + 6H2O(g) Heat = -904.4 kJ How does each of the following changes affect the yield of NO at equilibrium? Answer increase, decrease, or no change. a. increase [NH3] b. Increase [H2O] c. Decrease [O2] d. Decrease the volume of the container in which the raction occurs. e. Add a catalyst f. Increase temperature
18) Which of the following is an acid-base reaction? A) Fe(s) + 2 AgNO3(aq) - 2 Ag(s) + Fe(NO3)2(aq) B) MgSO4(aq) + Ba(NO3)2(aq) -- Mg(NO3)2(aq) + Baso C) C(s) + O2(g) - CO2(g) (D) 2 HCIO 4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(C1O4)2 E) None of the above are acid base reactions. 1 Determine the oxidation state of P in PO 33-. A-3 B) 0 C) +6
Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Mg2 ] = 0.774 M and [Sn2 ] = 0.0190 M. Standard reduction potentials can be found here. Reduction Half-Reaction Standard Potential Ered° (V) F2(g) + 2e– → 2F–(aq) +2.87 O3(g) + 2H3O+(aq) + 2e– → O2(g) + 3H2O(l) +2.076 Co3+(aq) + e– → Co2+(aq) +1.92 H2O2(aq) + 2H3O+(aq) + 2e– → 2H2O(l) +1.776 N2O(g) + 2H3O+(aq) + 2e– → N2(g) + 3H2O(l) +1.766 Ce4+(aq) + e– → Ce3+(aq)...
Name: 1. An exothermic reaction is allowed to reach equilibrium. If the temperature of the reaction mixture is decreased, the equilibrium will shift towards the product side: True False [1pt] 2. For the reaction C(s) + H2O(g) CO(g) + H2(g) a decrease in concentration of C(s) will cause the reaction to shift to the left oTrue False [1pt] 3. Define the following terms: [1.5pts] a. Activation Energy b. Exothermic Reaction c. Equilibrium [1p) 4. Determine the equilibrium constant K C(s)...
5) The Keq for the equilibrium below is 0.112 at 700.0°C S02 (8) 20269) 503 (Ⓡ) What is the value of Keq at this temperature for the following reaction? 1502(e) +40268) 2 03 () A) 5.60 10-2 B) 3.35 x 10-1 C) 1.79 101 D) 0.112 E) 2.99 6) The addition of HCl and to water produces a buffer solution. A) KOH B) HNO3 C) NH3 D) HC6H5OE) KNO3 7) The rate law for a reaction is rate = k[A][B]...