If you react 1 mole of zinc with a copper (II) nitrate solution, how many moles of copper preciptate do you have?
I assume this is "1", but I'm confused about if I need to know the number of moles of the copper (II) nitrate solution or not?
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2. When zinc metal reacts with copper(II) nitrate, zinc(II) nitrate and copper metal are the products. How many grams of zinc metal are required to react completely with 725 mL of 0.1955 M copper (II) nitrate solution? What mass of copper metal is produced? You will need a balanced equation to solve this problem! 3. One step in the process of manufacturing nitric acid (HNO3), a staple industrial chemical, is 3 NO2 (g) + H20 (1) ► 2HNO3...
1. When mixed, solutions of silver nitrate, AgNO, and sodium phosphate, Na3PO4, will form a precipitate of silver phosphate, Ag2PO4. The balanced equation is: 3AgNO3(aq) + Na3PO4(aq) Ag3PO4(s) + 3NaNO3(aq) Which of the following statements regarding this reaction is incorrect? A. 6 moles of AgNO, will react with 2 moles of Na2PO4 B. 9 moles of AgNO3 will form 2 moles of Ag3PO4, given sufficient Na3PO4 C. 1.5 moles of NaNO, will be formed when 0.5 mole of Na PO,...
Consider zinc hydroxide. It can be formed when solutions of zinc nitrate and sodium hydroxide are mixed. Its Ksp is 4.0x10-17. a) Write the equilibrium balanced equation and the Ksp equilibrium expression equation for zinc hydroxide. b) How many moles of sodium hydroxide must be added to 575 mL of 0.0300 M zinc nitrate to just start the precipitation of zinc hydroxide? c) Will a precipitate form if 10.00 mL of 0.0200 M NaOH is added to 250 mL of...
2. Assume you start with a 2.00 g sample of copper (II) nitrate. a. How many moles of copper (II) nitrate do you start with? b. Your sample will undergo multiple steps, each of which has the potential for loss of product. Assuming a percent yield of only 65.0 %, how many moles of copper (II) sulfate would you expect to produce? c. If the product is now dissolved in water inside of a 50-mL volumetric flask (as in the...
7. Solid zinc and aqueous copper (II) bromide react in a single replacement reaction producing zinc bromide and solid copper. How many grams of solid zinc nuggets must be put into this reaction in order to recover 25.0 grams of solid copper metal. (Assume 100% yield.)
Nitric acid and zinc react to form zinc nitrate, ammonium nitrate, and water. 4 Zn(s) + 10 HNO3(aq) - 4 Zn(NO3)2(aq) + NH4NO3(aq)+ 3 H20(0) (a) How many atoms of zinc react with 1.05 g HNO3? atoms (b) Calculate the number of grams of zinc that must react with an excess of HNO3 to form 28.3g NH4NO3
you need to make 2.00 L of 0.05 M copper (II) nitrate solution. How many grams of copper (II) nitrate will you require?
In lab, you reacted copper metal with aqueous nitric acid to produce aqueous Copper (11) nitrate, nitrogen dioxide gas and water. Cu (s) + 4HNO3 (aq) ---- > Cu(NO3)2 (aq) + 2NO2 (g) + 2H20 (1) a) If 0.210 gram of copper is reacted with 35.0 mL of 0.551 mol/L nitric acid, how many molecules and how grams of copper (II) nitrate are produced? b) How many moles of the reagent that is in excess are left over? c) If...
#13 Write a chemical equation for the reaction of zinc metal with aqueous copper (II) nitrate to produce aqueous zinc (II) nitrate and copper metal. #17 Potassium chlorate decomposes to potassium chloride and oxygen, as shown in the equation below. 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g) How many grams of oxygen are produced if 148 grams of potassium chloride are produced from the decomposition of 244 grams of potassium chlorate? #18 If the student collected...
In lab, you reacted copper metal with aqueous nitric acid to produce aqueous copper (II) nitrate, nitrogen dioxide gas and water. Cu (s) + 4HNO3 (aq) ---- > Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) a) If 0.210 gram of copper is reacted with 35.0 mL of 0.551 mol/L nitric acid, how many molecules and how grams of copper (II) nitrate are produced? b) How many moles of the reagent that is in excess are left over? c) If...