Topic: Sulfuric Acid. Disscuss the stregth of the acid, its realtive conductivity, pH, stability of the negative anion (conjugate base), polarity of the acid, and stregth of the H-A bond for Sulfuric Acid.

An ionic compound formed by a cation of radius 120pm and an anion radius 230pm will probably form a: (hint: calculate the difference in radius of cation and anion, compare to the examples in the "Course Materials")

What precautions should you take when working with strong acids?

Consider 1.70 mol of carbon monoxide and 2.60 mol of chlorine sealed in a 6.00 L container at 476 ^oC. The equilibrium constant, K_c, is 2.50 (in M^-1) for

CO(g) + Cl₂(g) ? COCl₂(g)

Calculate the equilibrium molar concentration of CO.

How much energy is required to raise the temperature of 100g of water from -10 to 110°C?

Write the principal equilibrium reaction and calculate the equilibrium constant for the base hydrolysis reaction of solid calcium phosphate to form monohydrogenphosphate anion as the principal phosphate containing species. Determine the pH of the solution. Ksp = 1.2 x 10-26. For H3PO4, Ka1, Ka2, and Ka3 = 7.5 x10-3 , 6.2 x 10-8 , and 4.8 x 10-13)

in one paragraph, discribe how the human body and/or its processes act like an electrolytic cell and voltaic cell. Include at least one chemical equation.

Suppose 0.234g of potassium bromide is dissolved in 50.mL of a 25.0mM aqueous solution of silver nitrate. Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the potassium bromide is dissolved in it. Be sure your answer has the correct number of significant digits. (M)

please only do if you are 100% sure, the pass three iv sent in have been wrong

1. Calculate the pH of a 0.17 M solution of HClO, with K_a = 3.5x10^{−8}.

2. At 25°C, 2.29E0 grams of sodium hydroxide is dissolved in enough water to make 500. mL of solution. Calculate ​[H_3O^+]. Do not enter units as part of your answer.

1. Explain the fragment patterns, isotope peaks, peak abundances, (The molecular formula for the compound is: C₂H₂Cl₂).

3:1 Ratio = Chlorine present

M⁺ peak

M⁺² peak

M⁺⁴ peak

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Please answer and show all work and units. Will rate ASAP.

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Consider the reaction shown below taking place at 25oC

N2(g) + 3 H2 (g) ⇆ 2 NH3 (g)

For this reaction it has been found that ∆Horx = - 92.38 kJ and ∆Sorx= - 98.4 J/K

A) Calculate the value of ΔGorx. Is this reaction spontaneous? Why or why not?

B) Calculate the value of the equilibrium constant, Kp, for this reaction. In which direction is the equilibrium displaced?

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Find out what you can about gel permeation chromatography (GPC). This technique is based on a different property of the compounds being separated than is thin-layer or traditional column chromatography. What property is this?

Show how the ratios of the simulated spherical S to the experimental S is equivalent to f/f0, and calculate this value. What does this suggest about the structure of the nuclesomal array in the saltfree buffer?

What are two different chemicals that we have added to the carbon cycle that did not previously exist naturally.

i.  Which functional group does each chemical belong to? Explain.

ii. How does the type of bonding and functional group these molecules posses affect their reactivity?

iii.   What are the health and environmental effects of the two chemicals?

Using the given data, calculate the change in Gibbs free energy for each of the following reactions. In each case indicate whether the reaction is spontaneous at 298 K under standard conditions.

Part A: 2Ag (s) + Cl2 (g) --> 2AgCl (s) Gibbs free energy for AgCl (s) is -109.70 kJ/mol

Part B: spontaneous or nonspontaneous

Part C: P4O10 (s) + 16H2 (g) --> 4PH3 (g) + 10H2O (g)

Gibbs free energy for P4O10 (s) is -2675.2 kJ/mol

Gibbs free energy for PH3 (g) is 13.4 kJ/mol

Gibbs free energy for H2O (g) is -228.57 kJ/mol

Part D: spontaneous or nonspontaneous

Part E: CH4 (g) + 4F2 (g) --> CF4 (g) + 4HF (g)

Gibbs free energy for CH4 (g) is -50.8 kJ/mol

Gibbs free energy for CF4 (g) is -635.1 kJ/mol

Gibbs free energy for HF (g) is -270.70 kJ/mol

Part F: spontaneous or nonspontaneous

Part G: 2H2O2 (l) --> 2H2O (l) + O2 (g)

Gibbs free energy for H2O2 (l) is -120.4 kJ/mol

Gibbs free energy for H2O (l) is -237.13 kJ/mol

Part H: spontaneous or nonspontaneous