Question

Two chemicals, A and B, react according to the following equation: A(aq) + 2 B(aq) ⟶ AB2(aq) Suppose that the reaction between 40.0 mL of 0.0135 M A(aq) and 50.0 mL of 0.0215 M B(aq) resulted in 0.000376 moles of AB2. Calculate the moles of A and B initially present before the reaction. mol A mol B Answer the following questions assuming the reaction went to completion. a. Given the amounts of reactants that were mixed, determine which should be the limiting reactant? A is the limiting reactantB is the limiting reactant b. Theoreticially, how many moles of AB2 would have been produced? mol c. What is the actual percent yield? Hint: % Answer the following questions assuming the reaction reached equilibrium. Using the moles of reactant initially present and the moles of product that actually formed, Hint: a. How many moles of A and B are left unreacted? mol A mol B b. Calculate Keq for the reaction. To do this, three molar concentrations will need to be calculated. First, divide each number of moles (A remaining, B remaining, AB2 formed) by the total volume of 0.0900 L using the equation below. Then, find Keq. Hint: m o l a r i t y = m o l e s l i t r e m o l a r i t y = m o l e s l i t r e Keq = When more of the reactant-in-excess was added to the reaction mixture, it was found that significant additional product was formed, Based upon this observation, did the reaction go to completion or reach equilibrium? completion equilibrium

Answer 1

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