The standard reaction free energy AGº =−1181. kJ for this reaction: 4 H2O2(1) + PbS(s)→PbSO (s) + 4 H2O(l) Use this information to complete the table below. Round each of your answers to the nearest kJ. 1 reaction 0 Δε ☐ x10 + PbS(s) ☐ kJ □kJ OkJ ±±ÞÚSО (s) + H2O (l) → H₂O₂(1) + -PbSO 4 2H₂O₂ (1) + ½ ½ Pbs (s) + ½ ½³bs (s) + 2H₂O(1) → -PbSО 2 4 PbSО(s) + 4H2O(l) → 4H₂O₂ (1) + PbS(s) ☑ The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH 3 is a weak base. acids: 0.7 mol of HCl is added to 1.0 L of a 0.4M NH3 solution. bases: ☐ ☑ other: ☐ 0.46 mol of HNO3 is added to 1.0 L of a solution that is 1.0M in both NH3 and NHBr. acids: bases: ☐ other: ☐ 0,0,...
The standard reaction free energy AGº =−1181. kJ for this reaction: 4 H2O2(1) + PbS(s)→PbSO (s) + 4 H2O(l) Use this information to complete the table below. Round each of your answers to the nearest kJ. 1 reaction 0 Δε ☐ x10 + PbS(s) ☐ kJ □kJ OkJ ±±ÞÚSО (s) + H2O (l) → H₂O₂(1) + -PbSO 4 2H₂O₂ (1) + ½ ½ Pbs (s) + ½ ½³bs (s) + 2H₂O(1) → -PbSО 2 4 PbSО(s) + 4H2O(l) → 4H₂O₂ (1) + PbS(s) ☑ The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH 3 is a weak base. acids: 0.7 mol of HCl is added to 1.0 L of a 0.4M NH3 solution. bases: ☐ ☑ other: ☐ 0.46 mol of HNO3 is added to 1.0 L of a solution that is 1.0M in both NH3 and NHBr. acids: bases: ☐ other: ☐ 0,0,...
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 50QRT
Related questions
Question
18- can you please help me with these 2 parts please? thank you!
![The standard reaction free energy AGº =−1181. kJ for this reaction:
4 H2O2(1) + PbS(s)→PbSO (s) + 4 H2O(l)
Use this information to complete the table below. Round each of your answers to the nearest kJ.
1
reaction
0
Δε
☐ x10
+
PbS(s)
☐ kJ
□kJ
OkJ
±±ÞÚSО (s) + H2O (l) → H₂O₂(1) +
-PbSO 4
2H₂O₂ (1) + ½ ½ Pbs (s) + ½ ½³bs (s) + 2H₂O(1)
→
-PbSО
2
4
PbSО(s) + 4H2O(l) → 4H₂O₂ (1) + PbS(s)
☑](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7bc30bfd-54a4-45be-8be6-a7bac17a47af%2Ff15a5e4c-49d1-4a35-8f8f-476a7de7f2e8%2Fdc5kgp_processed.png&w=3840&q=75)
Transcribed Image Text:The standard reaction free energy AGº =−1181. kJ for this reaction:
4 H2O2(1) + PbS(s)→PbSO (s) + 4 H2O(l)
Use this information to complete the table below. Round each of your answers to the nearest kJ.
1
reaction
0
Δε
☐ x10
+
PbS(s)
☐ kJ
□kJ
OkJ
±±ÞÚSО (s) + H2O (l) → H₂O₂(1) +
-PbSO 4
2H₂O₂ (1) + ½ ½ Pbs (s) + ½ ½³bs (s) + 2H₂O(1)
→
-PbSО
2
4
PbSО(s) + 4H2O(l) → 4H₂O₂ (1) + PbS(s)
☑
![The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at
equilibrium. You can leave out water itself.
Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the
formulas of the species that will act as neither acids nor bases in the 'other' row.
You will find it useful to keep in mind that NH 3 is a weak base.
acids:
0.7 mol of HCl is added to
1.0 L of a 0.4M NH3
solution.
bases: ☐
☑
other: ☐
0.46 mol of HNO3
is added
to 1.0 L of a solution that is
1.0M in both NH3 and
NHBr.
acids:
bases: ☐
other: ☐
0,0,...](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7bc30bfd-54a4-45be-8be6-a7bac17a47af%2Ff15a5e4c-49d1-4a35-8f8f-476a7de7f2e8%2Fijf9nmh_processed.png&w=3840&q=75)
Transcribed Image Text:The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at
equilibrium. You can leave out water itself.
Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the
formulas of the species that will act as neither acids nor bases in the 'other' row.
You will find it useful to keep in mind that NH 3 is a weak base.
acids:
0.7 mol of HCl is added to
1.0 L of a 0.4M NH3
solution.
bases: ☐
☑
other: ☐
0.46 mol of HNO3
is added
to 1.0 L of a solution that is
1.0M in both NH3 and
NHBr.
acids:
bases: ☐
other: ☐
0,0,...
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