2. (10 pts) Determine , and when 100.0 g of hydrogen reacts with sufficient amount of nitrogen to form ammonia at standard thermodynamic conditions. Determine Δ H, ΔU , ΔA , ΔG ,ΔS , q and w. The enthalpies of formation and entropies are: ΔHf = { H2= 0, N2 =0, NH3 =-46.1} Sْ = { H2 =130.68 , N2 = 191.61 , NH3 = 192.45 }

Which species has a normal boiling point closest to the normal boiling point of argon, Ar? (A) H2 (B) N2 (C) F2 (D) Cl and why

When 1.95 grams of Co(NO3)2 is dissolved in 0.750 L of 0.220 M KOH, what are the [Co 2+], [Co(OH)4 2-], and [OH-] if Kf of Co(OH)4 2- = 5.00x10^9?

Which of the following descriptions and/or equations best represents the enthalpy change of a system? There may be more than one correct answer.

A. The heat absorbed or released during a phase change or chemical reaction at constant pressure

B. The work done on or by a phase change or chemical reaction at constant pressure

C. deltaH = deltaE + PdeltaV

D. deltaE = q + w

E. H= E + PV

F. The heat sborbed or released during a phase change or chemical reaction at constant volume

G. The amount of energy required to raise the temperature of 1 mole of a substance by 1 degree C at constant pressure

H. The sum of the internal energy and the pressure-volume product of a system

For each of the following reactions provide a balanced chemical equation suppose exactly 5.00g of each reactant is taken. Determine which reactant is limiting and calculate what mass of each product is expected . (Assume that the liminting reactant is completely consumed).

identify the oxidizing agent in the reaction: Fe(s)+Cu(No3)2(aq)->Fe(NO3)2(aq)+Cu(s)

Determine the pH at the equivalence point for the titration of 40.0 mL of 0.1 M HNO2 by 0.200 M KOH. (The pK_a of nitrous acid is 3.36.)

Section A

1. Explain what happens to the pH paper in each of the following cases, and whether the substance is acid or base.

(a) Dry pH paper, household ammonia

(b) Moist pH paper, household ammonia

(c) Bleach

(d) Ammonium carbonate

2. Why are most cleaning agents and detergents basic?

Section B

3. What happens when you mix baking soda with vinegar? Describe your observations and write a balanced chemical equation to explain them.

4. What do you think would happen if you mixed the baking soda with concentrated sulfuric acid instead? What differences would you expect and why? Write and explain a balanced chemical equation for this reaction.

Section C

5. Do you see a trend in the periodic table that is related to the trend in the conductivity measurements? Explain why this trend occurs.

Section D

8. Explain your observations for Na vs. Ca in water. Write properly balanced chemical equations for the reactions, and explain the differences in your observations between the two elements based on their locations on the periodic table.

Section E

9. Explain how your observations relate to the positions of each element in the periodic table.

Section F

10. Explain how the reactivity with acid relate to the location of each substance on the periodic table.

Thank you so much!!!! :)

compare the rreducing capability of Lithium,Almunium hydride to those of sodium borohydride??

Physical Chemistry

A)The electrolytic conductivity of 0.10 M solution of acetic acid
is 5.3x 10-5 Scm-1. The cell constant was 0.10 cm-1. Neglecting activity
coefficient, Calculate the acid dissociation constant (Ka).
(Λmo for acetic acid = 390. S cm2 mol-1)

B)The observed osmotic pressure of 0.1 M acetic acid solution is
2.45 atm at 25.0 oC. Calculate the Van’t Hoff factor (i) and the degree of
ionization (α). Compare your value with that obtained from problem 1.
Comment on your answer.

An unknown compound contains only C, H, and O. Combustion of 3.90 g of this compound produced 9.18 g of CO2 and 2.51 g of H2O.

What is the empirical formula of the unknown compound?

Calculate the vapor pressure of a solution containing 25.3 g of glycerin (C3H8O3) in 119 mL of water at 30.0 ∘C. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerin is not volatile and dissolves molecularly (i.e., it is not ionic) and use a density of 1.00 g/mL for the water.

The boiling point of water is 100.0°C at 1 atmosphere.

How many grams of iron(II) chloride (126.8 g/mol), must be dissolved in 217.0 grams of water to raise the boiling point by 0.450°C? Refer to the table for the necessary boiling or freezing point constant.

The following half-reactions combine to make an electrolytic cell:

K+ (aq) + e-  K (s) E0 = −2.93

Li+ (aq) + e-  Li (s) E0 = −3.05

If a current of 1.5 Amps is placed on this cell for 5 minutes, which of the following describes the mass of solid formed (in grams) and the voltage required of the current. [1 Amp = 1 coul/s; 96500 coul = 1 mol e-]