5. What is the maximum amount of water that can be obtained from 22.05 g of copper and 750.00 mL of 1.00 M of nitric acid according to the below reaction? 3 Cu(s) + 8 HNO3(aq) → 3 Cu(NO3)2(aq) + 2 NO(g) + 4 H20(t)

Q: Explain the formula:   Ccal ΔTcal + mCpΔTwater + qrxn = 0

A:

Q: How many moles of precipitate will be formed when 260.0 mL of 0.200 M NaBr is reacted with excess…

A: Given : Molarity of NaBr = 0.200 M              Volume of solution = 260 mL To find : moles of PbBr2…

Q: 0.7532 g of copper turnings (molar mass: 63.546 g∙mol–1) are reacted with excess nitric acid.…

A: Disclaimer: In order to obtain copper sulfate the acid used in excess should be sulfuric acid and…

Q: How many grams of AgCl will be formed when 60.0 mL of 0.500 M AgNO₃ is completely reacted according…

A: Balanced Reaction FeCl₃ (aq) + 3AgNO₃(aq)→3AgCl (s) + Fe(NO₃)₃( aq) 3 mol AgNO3 prodcues 3 mol AgCl

Q: What quantity in moles of precipitate will be formed when 56.2 mL of 0.250 M AgNO3 is reacted with…

A: The volume of AgNO3 is .The molarity of AgNO3 is .The given balanced chemical equation is .To find…

Q: The amount of lead ion in a solution can be determined by gravimetric analysis using chemical…

A:

Q: Consider the reaction below. What are the spectator ions in this reaction? 3 Pb(NO3)2 (aq) + 2 FeCl3…

A: Spectator ions

Q: Consider the reaction of 45.0 mL of 0.355 M copper nitrate with 0.246 g of Aluminum metal. What is…

A: Limiting reagent is decided the amount of product

Q: 3. If 0.0275 L of 3.5 x 102 M Ba(OH)2 solution is needed to neutralize 10.0 mL of nitric acid…

A:

Q: What quantity in moles of precipitate will be formed when 45.1 mL of 0.250 M AgNO₃ is reacted with…

A:

Q: What quantity in moles of precipitate will be formed when 73.0 mL of 2.00 M NaI is reacted with…

A: Given reaction is, 2NaI(aq) + Pb(NO₃)₂(aq) → PbI₂(s) + 2NaNO₃(aq) From the given reaction, we can…

Q: What quantity in moles of precipitate will be formed when 272.5 mL of 0.400 M NaI is reacted with…

A:

Q: 2) N22CO3(aq) + CaCl2(aq) → 2 NaCl(ag) + CaCO3(s) Calculate the volume (in mL) of 0.200 M CAC12…

A: Given,Na2CO3aq +CaCl2aq →2 NaClaq+CaCO3s    Molarity of CaCl2=0.200M    Mass of CaCO3=2.00g    Molar…

Q: What mass of precipitate (in g) is formed when 250.0 mL of 0.110 M CdCl2 is mixed with excess KOH in…

A:

Q: How many liters of 0.15 M KCl solution are needed to completely react with 5.53 L of 0. 175 M lead…

A: The balanced chemical reaction is written below.2KCl (aq) + Pb(NO3)2 (aq) → PbCl2 (s) + 2KNO3…

Q: How many moles of precipitate will be formed when 70.0 mL of 2.00 M NaBr is reacted with 300.0 mL of…

A: The balanced chemical reaction:2NaBr(aq) + Pb(NO3)2(aq) → PbBr2(s) + 2NaNO3(aq)The volume of 2.00 M…

Q: How many moles of AgI will be formed when 75.0 mL of 0.300 M AgNO

A:

Q: What mass of precipitate (in g) is formed when 250.0 mL of 0.200 M CoCl₂ is mixed with excess KOH in…

A: The balanced equation is given as;   CoCl2(aq) + 2 KOH (aq)→Co(OH)2(s)+2KCl(aq) From the question,…

Q: Write the net ionic equation for the reaction shown. Include physical states. 2 HNO3(aq) +…

A: The reaction is given and we have to find out the net ionic equation of the given reaction.

Q: Na,CO3(aq) + CaCl,(aq) → 2 NaCl(aq) + CaCO3(s) Calculate the volume (in mL) of 0.200 M Na»CO3 needed…

A: Given, mass of CaCO3 = 2.00 g molar mass of CaCO3 = 100.09 g/mol => moles of CaCO3 = mass of…

Q: What quantity in moles of precipitate will be formed when 77.1 mL of 0.150 M AgNO3 is reacted with…

A:

Q: Consider the following unbalanced equation: AgNO3 (aq) + CaCl2 (aq) → AgCl (s) + Ca(NO3)2 (aq) How…

A: Given: 100.0 mL of 0.20 M silver nitrate reacts with 100.0 mL of 0.15 M calcium chloride. AgNO3 (aq)…

Q: What quantity in moles of precipitate will be formed when 73.7 mL of 0.150 M AgNO₃ is reacted with…

A:

Q: If 19.5 g of NaOH is added to 0.800 L of 1.00 M Zn(NO₃)₂, how many grams of Zn(OH)₂ will be formed…

A: Given, Mass of NaOH = 19.5 g            Molarity of Zn(NO₃)₂ = 1.00 M            Volume of Zn(NO₃)₂…

Q: According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 mL of 0.227 M…

A: Moles of LiOH used =Molarity of LiOH×Volume of LiOH= 0.227 mol/L×175.0×10-3L=0.0397 mol

Q: How many moles of precipitate will be formed

A: Molarity = number of moles/volume of solution (in L)  Number of moles = molarity × volume (in L)

Q: What mass of precipitate (in g) is formed when 20.5 mL of 0.700 M Zn(NO₃)₂ reacts with 23.0 mL of…

A: Number of moles of substance=Concentration of substance x Volume of substanceFor…

Q: How many moles of precipitate will be formed when 81.2 mL of 0.300 M AgNO₃ is reacted with excess…

A: According to the balanced chemical equation, 2 moles of AgNO3 gives 2 moles of AgI (precipitate).…

Q: How many moles of precipitate will be formed when 80.0 mL of 2.00 M NaI is reacted with 100.0 mL of…

A: 2 NaI (aq) + Pb(NO₃)₂ (aq) → PbI₂ (s) + 2 NaNO₃ (aq) To determining limiting reactant ; Firstly we…

Q: What quantity in moles of precipitate will be formed when 70.0 mL of 0.150 M AgNO₃ is reacted with…

A: Consider the given reaction is as follows; 2 AgNO3 (aq) + CaCl2 (aq) → 2 AgCl (s) + Ca(NO3)2 (aq)…

Q: 50.0 mL of a 1.25 M solution of nitric acid is added to 1.30 g of solid iron(III) hydroxide, what is…

A: Given that the 50 m L of 1.25 M solution of nitric acid is added to 1.30 g of iron(iii)hydroxide.

Q: How many moles of precipitate will be formed when 30.0 mL of 0.450 M AgNO₃ is reacted with excess…

A:

Q: What mass of precipitate (in g) is formed when 20.5 mL of 0.700 M Zn(NO₃)₂ reacts with 31.0 mL of…

A: ZnNO32+2 NaOH→ZnOH2 s+2 NaNO3 aqStength of ZnNO32=20.5x0.700 M1000=0.0143Stength of NaOH=310x0.700…

Q: Consider the reaction: 2A(aq)+B(aq)→C(aq) What is the limiting reactant if we mix equal volumes…

A:

Q: Consider the following unbalanced equation: AgNO3 (aq) + CaCl2 (aq) → AgCl (s) + Ca(NO3)2 (aq) How…

A:

Q: 2 Fe(OH);(s) + 3 H,SO,(aq) → Fe,(SO,)3(aq) + 6 H,O(1) a) In the first trial, she attempted to…

A: To do the calculations , we would use dimensional analysis method . We would consider the mole ratio…

Q: What mass of precipitate (in g) is formed when 250.0 mL of 0.285 M MnCl₂ is mixed with excess KOH in…

A: Mass of precipitate of Mn(OH)2 formed is 6.269g.

Q: How many moles of precipitate will be formed when 69.3 mL of 0.300 M AgNO₃ is reacted with excess…

A: Given, 69.3 mL of 0.300 M AgNO₃

Q: How many moles of precipitate will be formed when 200.0 mL of 0.400 M NaI is reacted with excess…

A:

Q: How many grams of AgCl will be formed when 60.0 mL of 0.500 M AgNO₃ is completely reacted according…

A:

Q: 1. A 25.0 mL of Ba(OH)2 of unknown concentration was placed in the Erlenmeyer flask. A titration was…

A: From the given balanced reaction we can see that the 2 moles of HNO3 is required to completely…

Q: . For the following reaction, how many mL of 0.200 M NaOH solution are needed to react with 18.0 mL…

A: Given - Molarity of NaOH - 0.200M Molarity of NiCl2  - 0.500M Volume of NiCl2 - 18 ml = 0.0180 L To…

Q: What quantity in moles of precipitate will be formed when 100.0 mL of 2.00 M NaI is reacted with…

A:

Q: 60.5 mL of HNO3 is required to react with 25.0 mL of a 1.00 M Barium hydroxide solution: Find the…

A: Given- Volume of HNO3=60.5 mL  Volume of barium hydroxide= 25.0mL Molarity of barium hydroxide=…

Q: How many moles of precipitate will be formed when 154.5 mL of 0.350 M NaCl is reacted with excess…

A:

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".