12. What amount (in mol) and what mass (in g) of zinc(II) sulfate can be produced whe copper(II) sulfate reacts with 484 g of zinc? CuSO4 (aq) + Zn(s) → Cu(s) + ZnSO, (ag) A: 2.71;

What mass of precipitate (in g) is formed when 45.5 mL of 0.300 M Na₃PO₄ reacts with 58.5 mL of 0.200 M CrCl₃ in the following chemical reaction? Na₃PO₄(aq) + CrCl₃(aq) → CrPO₄(s) + 3 NaCl(aq)

1. For each of the following reactions, identify the category of reaction, balance reaction, and describe how you knew a reaction took place. To indicate an already balanced reaction, write balanced above the reaction. Reaction 1 Balance: H2O(1) + NO2(g) Cu(s) Cu(NO3)2(aq) + HNO3(aq) + Reaction Category: How did you identify a reaction took place? Reaction 2 Balance: Cu(NO3)2(aq) + NaOH(aq) – Cu(OH)2(s) + NaNO3(aq) Reaction Category: How did you identify a reaction took place? OhoW Reaction 3 Balance: Cu(OH)2(s) → CuO(s) + H2O(1) Reaction Category: How did you identify a reaction took place? Reaction 4 Balance: CuO(s) + H2SO4(aq) – CuSO4(aq) + H2O() Reaction Category: How did you identify a reaction took place? Reaction 5 Balance: CuSO4(aq) + Zn(s) → ZNSO4(aq) + Cu(s) Reaction Category: How did you identify a reaction took place?

4.106. Aspirin (acetlsalicyclic acid) may be formed from salicyclic acid and acetic acid as follows:C7H6O3 (aq) + CH3COOH (aq)  → C9H8O4(s) + H2O(l)Salicyclic acid    Acetic Acid               Aspirin b. How many mol of aspirin may be produced from 1.00*102 mol mol salicylic acid? c. How many g of aspirin may be produced from 1.00*102 mol salicylic acid? d. How many g of acetic acid would be required to completely with the 1.00*102 mol salicylic acid? e. For the conditions in part (d), how many g of aspirin would form?

2. Given that 0.0643 mol Mg(OH)2 (58.32 g/mol) are theoretically formed in the reaction: 2 NaOH (aq) + MgCl2 (aq)  2 NaCl (aq) + Mg(OH)2 (s) calculate the percent yield of Mg(OH)2 (s) if you weighted the product at the end of the experiment and your actual yield is 3.18g.

Addition of NaOH to a Cu(NO3)2 solution results in the precipitation of Cu(OH)2.               2 NaOH     +     Cu(NO3)2     à     Cu(OH)2 (s)     +     2 NaNO3           If 10.00 g if NaOH is added to a solution that contains 25.00 g of Cu(NO3)2, what is the limiting reagent?  How many grams of Cu(OH)2 are produced?

Iodine is prepared both in the laboratory and commercially by adding Cl2(g) to an aqueous solution containing sodium iodine 2Nal(aq)+Cl2(g)---> I2(s)+2NaCl(aq)  How many grams of sodium iodide, NaI, must be used to produce 82.1 g of iodine, I2?

The following reaction takes place as represented by the balanced chemical equation below: 2 K3PO4 (aq)  +  3 Ba(NO3)2 (aq)  -->  6 KNO3 (aq)  +  Ba3(PO4)2 104.7 mL of a 2.50 M K3PO4 solution is reacted with an excess amount of Ba(NO3)2 solution. How many grams of Ba3(PO4)2 should be produced? Numerical answer:   Unit:   Label:  Ba3(PO4)2

In the following reaction, 35.0 mL of 0.150 M magnesium bromide solution reacts with excess silver nitrate to form a precipitate. What is the expected mass of AgBr in grams? (molar mass of AgBr = 187.77 g/mole) MgBr2(aq) + 2AgNO3(aq) --> 2AgBr(s) + Mg(NO3)2(aq)   Question 11 options:   0.985 g   0.493 g   1.97 g   986 g   none of these

O 000 How many grams of HCl can react with 0.750 g of Al(OH)3 according the following balanced equation? Molar masses: Al(OH)3= 78.01 g, AICI3= 133.33 g, HCI= 36.46 g Al(OH)3(s) + 3 HCI (aq) --> AICI3(aq) + 3 H2O 3.85 g 1.05 g 0.0288 g 1.32 g