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1) Evaluate the solubility of the following ionic substances.

  1. NaOH c. MgCO3 e. Ag2SO4
  2. PbCl2 d. K3PO4 f. CaSO4

Dr. Blackburn

g. Ba3(PO4)2

h. (NH4)2CO3

  1. 2) Predict the products that can form if the following aqueous reagents are mixed. This includes making sure the chemical formulas are charged balanced. Evaluate the solubility of the products and include the correct phase designations after the chemical formulas.
    1. KCl (aq) + Pb(NO2)2 (aq) à
    2. Na2SO4 (aq) + CaCl2 (aq) à
    3. MgSO4 (aq) + Na3PO4 (aq) à
    4. Na2S (aq) + CaCl2 (aq) à
  2. 3) Write the complete ionic equation for the following molecular equations.
    1. MgCl2(aq) + 2AgNO3(aq) →2AgCl(s) + Mg(NO3)2(aq)
    2. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)
    3. Na2SO4(aq) + Pb(NO3)2(aq) → PbSO4(s) + 2NaNO3(aq)
  3. 4) Write the net ionic equation for the following reactions.
    1. Na+(aq) + Cl ̄(aq) + Ag+(aq) + NO3 ̄(aq) ---> AgCl(s) + Na+(aq) + NO3 ̄(aq)
    2. 6Na+ (aq)+2PO43- (aq)+3Ca2+ (aq)+6Cl- (aq)-->6Na+ (aq)+6Cl- (aq)+Ca3(PO4)2 (s)
    3. 6NH4+ (aq)+3CO32- (aq)+2Al3+(aq)+6NO3-(aq)-->6NH4+ (aq)+6NO3- (aq)+Al2(CO3)3 (s)
    4. 2Na+ (aq)+2OH- (aq)+2H+ (aq)+SO42- (aq)-->2Na+ (aq)+SO42- (aq)+2H2O(l)

5) Use the following choices to classify each reaction given below (more than one choice may apply).

  1. oxidation-reduction
  2. neutralization (acid-base)
  3. precipitation

d. double displacement e. single displacement f. combustion

g. synthesis
h. decomposition

C3H8 (g) + O2(g) CO2 (g ) + H2O(g) Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq) Zr(s) + O2(g) → ZrO2(s)
6Na(s) + N2(g) → 2Na3N(s)

2Hg(l) + O2(g) → 2HgO(s) Ca(s) + H2(g) → CaH2(s) 8Fe(s)+S8(s)→8FeS(s) 2 KCl(s) → 2 K(s) + Cl2(g)

  1. ZnBr2(aq) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2AgBr(s)
  2. Na2SO4(aq) + Pb(NO3)2(aq) → PbSO4(s) + 2NaNO3(aq)
  3. HC2H3O2(aq) + CsOH(aq) → H2O(l) + CsC2H3O2(aq)
  4. HNO3(aq) + NaOH(aq) → H2O(l) + NaNO3(aq)
  5. H2SO4(aq) + Ba(OH)2(aq) → 2H2O(l) + BaSO4(s)
  6. 2HCl(aq) + Pb(OH)2(aq) → PbCl2(s) + 2H2O(l)
  7. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq)
  8. 2AgNO3(aq) + Zn(s) → 2Ag(s) + Zn(NO3)2(aq)

ix. x. xi. xii. xiii. xiv. xv. xvi.

6) Identify whether the following reactions are molecular equations, complete ionic equations, or net ionic equations.

  1. Cu2+(aq) + 2NO3-(aq) + 2Na+(aq) + 2OH-(aq) →Cu(OH)2(s) + 2Na+(aq) + 2NO3-(aq)
  2. Ba2+(aq) + SO42-(aq) →BaSO4 (s)
  3. HNO3(aq) + KOH(aq) →KNO3(aq) +H2O(l)
  4. Ba2+(aq) + 2OH-(aq) + 2H+(aq) + 2Cl-(aq) →2H2O(l) + Ba2+(aq) + 2Cl-(aq)

Chem 1104 Fall 2018 Worksheet #5 – Balancing Equations Name: ________________________________________ Due: 9/4/18 Dr. Blackburn 1) ____ Na3PO4 + ____ KOH à ____ NaOH + ____ K3PO4 2) ____ MgF2 + ____ Li2CO3 à ____ MgCO3 + ____ LiF 3) ____ P4 + ____ O2 à ____ P2O3 4) ____ RbNO3 + ____ BeF2 à ____ Be(NO3)2 + ____ RbF 5) ____ AgNO3 + ____ Cu à ____ Cu(NO3)2 + ____ Ag 6) ____ CF4 + ____ Br2 à ____ CBr4 + ____ F2 7) ____ HCN + ____ CuSO4 à ____ H2SO4 + ____ Cu(CN)2 8) ____ GaF3 + ____ Cs à ____ CsF + ____ Ga 9) ____ BaS + ____ PtF2 à ____ BaF2 + ____ PtS 10) ____ N2 + ____ H2 à ____ NH3 11) ____ NaF + ____ Br2 à ____ NaBr + ____ F2 12) ____ Pb(OH)2 + ____ HCl à ____ H2O + ____ PbCl2 13) ____ AlBr3 + ____ K2SO4 à ____ KBr + ____ Al2(SO4)3 14) ____ CH4 + ____ O2 à ____ CO2 + ____ H2O 15) ____ Na3PO4 + ____ CaCl2 à ____ NaCl + ____ Ca3(PO4)2 16) ____ K + ____ Cl2 à ____ KCl 17) ____ Al + ____ HCl à ____ H2 + ____ AlCl3 18) ____ N2 + ____ F2 à ____ NF3 19) ____ SO2 + ____ Li2Se à ____ SSe2 + ____ Li2O 20) ____ NH3 + ____ H2SO4 à ____ (NH4)2SO4
Chem 1104 Fall 2018 Worksheet #5b – Chemical Rxns Name: ________________________________________ Due Date: 10/9/18 Dr. Blackburn 1) Evaluate the solubility of the following ionic substances. a. NaOH c. MgCO3 e. Ag2SO4 b. PbCl2 d. K3PO4 f. CaSO4 g. Ba3(PO4)2 h. (NH4)2CO3 2) Predict the products that can form if the following aqueous reagents are mixed. This includes making sure the chemical formulas are charged balanced. Evaluate the solubility of the products and include the correct phase designations after the chemical formulas. a. KCl (aq) + Pb(NO2)2 (aq) à b. Na2SO4 (aq) + CaCl2 (aq) à c. MgSO4 (aq) + Na3PO4 (aq) à d. Na2S (aq) + CaCl2 (aq) à 3) Write the complete ionic equation for the following molecular equations. a. MgCl2(aq) + 2AgNO3(aq) → 2AgCl(s) + Mg(NO3)2(aq) b. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq) c. Na2SO4(aq) + Pb(NO3)2(aq) → PbSO4(s) + 2NaNO3(aq) 4) Write the net ionic equation for the following reactions. a. Na+(aq) + Cl¯(aq) + Ag+(aq) + NO3¯(aq) ---> AgCl(s) + Na+(aq) + NO3¯(aq) b. 6 Na+ (aq) + 2 PO43- (aq) + 3 Ca2+ (aq) + 6 Cl- (aq) --> 6 Na+ (aq) + 6 Cl- (aq) + Ca3(PO4)2 (s) c. 6 NH4+ (aq) + 3 CO32- (aq) + 2 Al3+ (aq) + 6 NO3- (aq) --> 6 NH4+ (aq) + 6 NO3- (aq) + Al2(CO3)3 (s) d. 2 Na+ (aq) + 2 OH- (aq) + 2 H+ (aq) + SO42- (aq) --> 2 Na+ (aq) + SO42- (aq) + 2 H2O (l) 5) Use the following choices to classify each reaction given below (more than one choice may apply). a. oxidation-reduction b. neutralization (acid-base) c. precipitation d. double displacement e. single displacement f. combustion g. synthesis h. decomposition i. ZnBr2(aq) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2AgBr(s) ix. C3H8 (g) + O2(g) à CO2 (g ) + H2O(g) ii. Na2SO4(aq) + Pb(NO3)2(aq) → PbSO4(s) + 2NaNO3(aq) x. Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq) iii. HC2H3O2(aq) + CsOH(aq) → H2O(l) + CsC2H3O2(aq) xi. Zr(s) + O2(g) → ZrO2(s) iv. HNO3(aq) + NaOH(aq) → H2O(l) + NaNO3(aq) xii. 6Na(s) + N2(g) → 2Na3N(s) v. H2SO4(aq) + Ba(OH)2(aq) → 2H2O(l) + BaSO4(s) xiii. 2Hg(l) + O2(g) → 2HgO(s) vi. 2HCl(aq) + Pb(OH)2(aq) → PbCl2(s) + 2H2O(l) xiv. Ca(s) + H2(g) → CaH2(s) vii. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq) xv. 8 Fe(s) + S8 (s) → 8 FeS (s) viii. 2AgNO3(aq) + Zn(s) → 2Ag(s) + Zn(NO3)2(aq) xvi. 2 KCl(s) → 2 K(s) + Cl2(g) 6) Identify whether the following reactions are molecular equations, complete ionic equations, or net ionic equations. 2+ + + a. Cu (aq) + 2NO3 (aq) + 2Na (aq) + 2OH (aq) → Cu(OH)2(s) + 2Na (aq) + 2NO3 (aq) 2+ b. Ba (aq) + SO42-(aq) → BaSO4 (s) c. HNO3(aq) + KOH(aq) → KNO3(aq) +H2O(l) d. Ba (aq) + 2OH (aq) + 2H (aq) + 2Cl (aq) → 2H2O(l) + Ba (aq) + 2Cl (aq) 2+ - + - 2+ -
Chem 1104 Fall 2018 Worksheet #6 – Molar Calculations Name: ________________________________________________ Due: 10/11/18 Dr. Blackburn Calculate the number of moles that correspond to following mass amounts of the given substances. 1) 56.0 g NaCl 2) 23.4 g MgSO4 3) 7.89 g Ni(OH)2 4) 45.24 g C3H8 5) 524 g C6H11OH 6) 589.43 g Ca3(PO4)2Ÿ2H2O Calculate the mass amount that corresponds to the following molar amounts of the given substances. 7) 12.45 mol CCl4 8) 0.725 mol As2O3 9) 5.78 mol CO2 10)0.984 mol Ar 11)1.245 mol H2O 12)27.534 mol Pb(SO3)2 Calculate the indicated quantity given the chemical equation and amount of substance. 13) How many grams of water will be produced from 1.325 g of C3H8? C3H8 + 5 O2 (g) à 3 CO2 + 4 H2O 14) How many grams of Fe3O4 will be produced from 34.65 g of Fe? 4 Ga2O3 + 9 Fe (s) à 3 Fe3O4 + 8 Ga (s) 15) How many grams of Al2(SO4)3 is needed produce 12.48 g of Al(OH)3? Al2(SO4)3 + 3 Ca(OH)2 à 2 Al(OH)3 + 3 CaSO4 16) How many grams of P4 is needed produce 125.63 g of P2O5? P4 + 5 O2 à 2 P2O5

Tutor Answer

remjius
School: UC Berkeley

Hello,Please find completed work.Let me know if you need any editing.Regards,Remjius.

Chem 1104

Fall 2018 Name: ________________________________________________

Worksheet #6 – Molar Calculations Due: 10/11/18 Dr. Blackburn
Calculate the number of moles that correspond to following mass amounts of the given
substances.
1) 56.0 g NaCl
56*1/58.5 =0.9573 moles
2) 23.4 g MgSO4
23.4*1/120 =0.195 moles
3) 7.89 g Ni(OH)2
7.89*1/92.5 = 0.0853 moles
4) 45.24 g C3H8
45.24*1/44 =1.0282 moles
5) 524 g C6H11OH
524*1/100 = 5.24 moles
6) 589.43 g Ca3(PO4)2.2H2O
589.43*1/330 = 1.7862 moles
Calculate the mass amount that corresponds to the following molar amounts of the given
substances.
7) 12.45 mol CCl4
Moles=mass/RFM
12.45*154 = 1917g
8) 0.725 mol As2O3
0.725*198 = 143.6g
9) 5.78 mol CO2

5.78*44 = 254.3g
10)0.984 mol Ar
0.984*40 = 39.4g
11)1.245 mol H2O
1.245*18 = 22.4g
12)27.534 mol Pb(SO3)2
27.534*367 = 10105g
Calculate the indicated quantity given the chemical equation and amount of substance.
13) How many grams of water will be produced from 1.325 g of C3H8? C3H8 + 5 O2 (g) → 3
CO2 + 4 H2O
1.325/44 = 0.03 moles
4*0.03 = 0.12 moles
Moles=mass/RFM
0.12*18 = 2.16g
14) How many grams of Fe3O4 will be produced f...

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