b. 8 HNO3 + 3 Cu 3 Cu(NO3)2 + 4 H2O + 2 NO -> 3.2 g IMoICh 3.29(4x 63. 55 gcu Molar Mass

Balance: HC2H3O2(aq)+ Al(OH)3(s)

16) According to the balanced chemical equation 5 H2C20 4(aq) + 2 MnO4-(aq) + 6 H+(aq) →10 CO 2(g) + 2 Mn2+(aq) + 8 H2O() 0.3500 grams of oxalic acid, H2C2O4 will react with_ _moles of permanganate, MnO4". A) 0.009718 B) 0.001554 C) 0.003887 D) 0.007774

9:06am ructions t to click Submit when completed! Question 17 Determine the molarity of a solution formed by dissolving 861 g of Mgl2 in enough water to yield 474 mL of solution. * Previous No new data to save. Last checked at 9:21am le Drive MacBook Air 80 888 esc F1 F2 F4 F5 F6 F7 @ 2$ 4 & 6. 7 8. Q W E R. T Y © 2N

Mercury can be obtained by reacting mercury(II) sulfide (show below) with calcium oxide. If you began with 136.6 grams of mercury(II) sulfide and mixed it with excess amounts of calcium oxide, how many moles of calcium sulfide will you make? 4 HgS (s) +4 CaO (s)--> 4 Hg (1)+3 CaS (s) +1 CaSO4 (s) round your answer using appropriate sig fig rules

In the reaction CrCl3 (aq) + 3 AgNO3 (aq) --> Cr(NO3)3 (aq) + 3 AgCI (s) 4.4 moles of CrClą are reacted with 1 moles of AgNO3. Determine the theoretical yield in mols of the product, silver chloride.

A chemist adds 2.00 L of a 5.9 × 10M mercury(II) iodide (HgI₂) solution to a reaction flask. Calculate the moles of mercury(II) iodide the chemist has added to the flask. Round your answer to 2 significant digits. mol 0 X S

2.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

3 Cu   +   8HNO3  --> 3 Cu(NO3)2    +  2 NO   +  4  H2O In the above equation how many moles of water can be made when 178.7 grams of HNO3 are consumed?

Chemists can produce silver metal by reacting copper metal with a solution of silver nitrate: Cu(s) + 2 AgNO3(aq) → 2 Ag(s) + Cu(NO3)2(aq) KAU YA (a) Predict the amount of silver produced if 0.24 mol of copper were combined with 0.52 mol of silver nitrate. (b) Predict the amount of excess reagent remaining.