If a solution containing 58 g of mercury(II) nitrate is allowed to react completely with a solution containing 16.642 g of sodium sulfate according to the equation below: Hg(NO3)2(aq)+Na2SO4(aq)------2NaNO3(aq)+HgSO4(s)   A. How many grams of solid precipitate will be formed if the reaction has a 100% yield? B. How many grams of the excess reagent will remain after the reaction? C. If the reaction has only an 80% yield, how many grams of solid precipitate will be formed?

Fe(II) can be precipitated from a slightly basic aqueous solution by bubbling oxygen through the solution, which converts Fe(II) to insoluble Fe(III): $$4Fe(OH)+(aq)+4OH−(aq)+O2​(g)+2H2​O(l)4Fe(OH)3​(s)  How many grams of O2 are consumed to precipitate all of the iron in 75.0 mL of 0.0350 M Fe(II)?

If 10.0g of copper reacts with 40.0g of silver (I) nitrate, determine the limiting reactant and the mass of silver and copper (II) nitrate formed in the reaction.  AgNO3 + Cu -> Ag + Cu(NO3)2

2) Balance the following chemical equation: Al(NO3)3 + Na2S Al,S3 + NANO, 3) If 10.0 mL of a 10.0 M stock solution of NaOH is diluted to 250 mL, what is the concentration of the resulting stock solution? 4) Decomposition of KCI03 is sometimes used to prepare small amounts of 02 in the laboratory. How many grams of 02 can be prepared from 4..50g of KC103? 2 KC1O3 (s) – 2 KCl (s) + 3 02 (g) English (United States) ng Exam 1 Review - 20. 84

The following precipitation reaction is perfomed using 3.785 g of FeCk and 2.258 g of NaOH. FeCk (aq) +3 NaOH (aq) Fe(OH): (s) 3 NaCl (ag) a. What is the theoretical yield of the produce (solid) in this reaction? b. If the reaction produces 1.825 g of the product, what is the percent yield? c. Write the full and net ionic equations for this reaction.

When 75.0 mL of a 1.20 M solution of magnesium iodide reacts with 80.0 mL of a 1.50 M solution of silver nitrate, how many grams of precipitate (solid) can be produced? Which reactant is in excess? MgI2 (aq)  +  2AgNO3 (aq)  -->  Mg(NO3)2 (aq)  +  2AgI (s) grams of precipitate:    ________g Excess reactant (provide name, not formula):  ___________

In the following balanced reaction: Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) 10.9 g of KI react with a 0.193 mol L-1 solution of Pb(NO3)2. The total solution volume is 0.200L If 8.31 g of PbI2 is collected, what is the percent yield?

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What element is being oxidized in  the following reaction.

An experimenter reacts 30.0 mL of a BaCl2 solution with excess AgNO3 as shown in the unbalanced equation below.  If 2.58 grams of AgCl are obtained, what is the molarity of BaCl2solution? Hint: First balance the chemical equation. BaCl2 (aq) + AgNO3 (aq) ---> Ba(NO3)2 (aq) + AgCl (s)