KClO₃ disproportionates on heating to give KCl and KClO₄ only. The number of moles of KClO₄ produced on complete disproportionation of 24.5 g KClO₃ is

• A. 0.156
• B. 0.106
• C. 0.126
• D. 0.206
• E. 0.056

Predict the sign of the entropy change for each of the following processes and give your reasoning why:

1. Solid sugar is added to water to form a solution.

2. Iodine vapor condenses on a cold surface to form crystals.

3. N₂(g) + 3H₂ (g) 2 NH₃(g)

4. H₂O(l) H₂O(g)

5. CaCO₃(s) CaO(s) + CO₂(g)

6. NH₄NO₃(s) + H₂O(l) NH₄⁺ (aq) + NO₃^- (aq)

7. freezing of water   

8. boiling of water

9. crystallization of salt from a supersaturated solution

10. the reaction 2 NO(g) → N2O2(g)

11. the reaction 2 H2(g) + O2(g) → 2 H2O(g)

12. Fe(s) → Fe(l)   

13. 2 Fe(s) + 3/2 O2(g) → Fe2O3(s)   

14. HF(l) → HF(g)

15. 2 H2O2(l) → 2 H2O(l) + O2(g)

16. H2O(l) -> 2 H2(g) + O2(g)

17. CO_(g) + 3 H_2(g)-> CH_4(g) + H₂O_(g)

18. 2 NaHCO_3(s) ---> Na₂CO_3(s) + H₂O_(g) + CO_2(g)

19. CO(g) + H₂O(g) ----> CO₂(g) + H₂(g)

20. CaCO₃(s) ----> CaO(s) + CO₂(g)

21. 2NH₃(g) + CO₂(g) ----> NH₂CONH₂(aq) + H₂O(l)

22. 2Na₂O₂(s) + 2H₂O(l) ---> 4NaOH(aq) + O₂(g)

23. C₂H₅OH(l) + 3O₂(g) ---> 2CO₂(g) + 3H₂O(g)

Plz let me know how you did it.

Simple description is the best

Thanks

Calculate E?cell for each of the following balanced redox reactions.

A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq)

B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s)

C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq)

D. Determine whether the reaction in part A is spontaneous as written.

E. Determine whether the reaction in part B is spontaneous as written.

F. Determine whether the reaction in part C is spontaneous as written.

Using standard Gibbs energy of formation values given in the table, calculate the equilibrium constant K of the reaction

Cl2_(g)+2NO_(g)⇌2NOCl_(g)

The standard Gibbs energy change of the reaction represents the drive the reaction has under standard conditions to move toward equilibrium from point A to point X in the diagram.

Substance	ΔfG∘ (kJ mol−1)
Cl2(g)	0
NO(g)	86.71
NOCl(g)	66.30

Nitrogen gas is compressed isothermally at 250K from 1.0 bar to 150 bars. Determine the change in enthalpy and entropy using:
a. Redlich-Kwong equation of state
b. Using tabular superheat data

nstant cold packs sometimes used to treat athletic injuries contain solid ammonium nitrate and liquid water separatedbya thin divider. When the divider is broken, the ammonium nitrate dissolves endothermically:

NH4NO3(s) NH4+(aq) + NO3–(aq)

To measure the enthalpy of this reaction, you dissolve 1.25 g of ammonium nitrate in enough water to make 25.0 mL of solution. The initial temperature is 25.8 °C, and the final temperature is 21.9 °C. (Assume that the density of the solution is 1.00 g /mL and that the heat capacity of the solution is 4.184 J/g∙°C

A student mixes 5.00 mL of 2.00 x 10‐3 M Fe(NO3)3 with 5.00 mL 2.00 x 10‐3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN+2 is 1.40 x 10‐4 M.

What is the initial concentration in solution of the Fe+3 and SCN‐?

What is the equilibrium constant for the reaction?

What happened to the K+ and the NO3‐ ions in this solution?

How many grams of O2 can be prepared from the thermal decomposition of 4.09kg of H2O

Titration: calculate (a) the initial pH, (b) the volume and the pH at 1/3 of the equivalence point, (c) the volume and the pH at 2/3 of the equivalence point, (d) the volume and the pH at 99/100 of the equivalence point, (e) the volume and the pH at the equivalence point, (f) the volume and the pH at 101/100 of the equivalence point, (g) the volume and the pH at 4/3 of the equivalence point, and (h) the volume and the pH at 5/3 of the equivalence point. The initial volume of acid is 1.00 L. Using 1.00L 0.2217M HIO Ka=2.3x10^-11 Titrated with 0.1443M KOH

Count Valence e-	Formula	Electron Geometry	Molecular Geometry
1 N = 5 3 H = 3 8 / 2 = 4 pair	NH3	Tetrahedral	Trigonal pyramidal
	H2O
	CBr4
	SO3 This is not a polyatomic ion … No charge!!!
	PI3
	CH3Cl Carbon is the central atom
	NO31-
	CO32-
	NH4+1
	CH4
	SO2

Consider the following unbalanced redox reaction

CrO₄^2- + (CH₃)H + H⁺ → Cr³⁺ + HCOOH + H₂O

Which of the following statements is/are correct?

1.CrO₄^2- is the oxidizing agent.

2. The oxidation number of Cr is decreased in the redox reaction.

3. Electrons are released from CrO₄^2-

• A. 1 only
• B. 1 & 3 only
• C. 2 & 3 only
• D. 1 & 2 only
• E. all

Juice is put into bottles and sealed. Each bottle contains 1500 mL of product and has 65 mL headspace of air with 20% by volume of oxygen in it. The specific gravity of the product is 1.04.

During packaging, the dissolved oxygen content of the product is 7.0 ppm. The juice concentrate contributes 5.5 mg Vitamin C per 100 mL to the final product mixture. The processor then adds an unknown amount of vitamin C to the product to bring it to the desired concentration after storage. After storage, the Vitamin C content of the product falls to 55 mg per 100 mL.  15.7mg of Vitamin C are needed to consume 1mL of oxygen.

How much Vitamin C (in grams) would the processor need to add to make enough beverage to fill 1,000 bottles?

1. From an evolutionary perspective, why does the fermentation pathway exist?
2. Given that generating pyruvate gives net 2 ATPs, what is the biochemical rationale for converting pyruvate to lactate?

Explain why ICP-MS is more sensitive than ICP-AES.

Calculate the pH of the solution that results from each of the following mixtures.

140.0mL of 0.26M HF with 220.0mL of 0.30M NaF