A solution is prepared by dissolving 50.8 g sucrose(C12H22O11) in 0.387 kg of water. The final volume of the solution is 355 mL.

For this solution, calculate molarity.

For this solution, calculate molality.

For this solution, calculate percent by mass.

For this solution, calculate mole fraction.

3. a) Using only the following information:   

• ∆H°f for NO (g) is +90.4 kJ/mol
   • ∆H° = –56.6 kJ/mol for the reaction: NO (g) + 1/2 O2 (g) à  NO2 (g)  

Determine ∆H°f for NO2 (g).

b) Using only your answer to (a) and the following information:    

•∆H° = –283.0 kJ/mol for the reaction: CO (g) + 1/2 O2 (g) à  CO2 (g)  Determine ∆H° for the reaction:   4 CO (g) + 2 NO2 (g) à  4 CO2 (g) + N2 (g)

c) A 10.0-L vessel contains 5.0 atm of CO and 3.0 atm of NO2 at 25°C. How much heat (in Joules) will be liberated if this is allowed to react to completion according to the reaction in part (b)?
d) In a separate experiment using a very large reaction vessel with a movable piston, 6.00 moles of CO2 (g) reacts completely with 3.00 moles of nitrogen gas according to the following equation at 25°C and with

a constant external pressure of 2.00 atm:

4 CO2 (g) + N2 (g) à  4 CO (g) + 2 NO2 (g)     
  This reaction proceeds to completion. Calculate ∆U, q, and w for this reaction under these conditions.

Pay attention to the ratio. An acid of pKa = 8.0 is present in a solution with a pH of 6.0. What is the ratio of protonated to the deprotonated form of the acid? Show your work

Classify this reaction.s this a synthesis, decomposition, single displacement or double displacement reaction?Acid Base? Redox? How do you know this?

Equation for chemiluminescence:

2K₃[Fe(CN)₆] + 2KOH + H₂O₂ → 2K₄[Fe(CN)₆] + 2H₂O + O₂

For the minimum and maximum allowed pH values of blood, calculate the following ratios (you may use relevant Ka values that are tabulated for 25C in Appendix D of your textbook):

[Species #1] / [Phosphoric Acid]

[Species #2] / [Phosphoric Acid]

[Species #3] / [Phosphoric Acid]

Appendix D says: Phosphoric Acid H3PO4 Ka1 7.5 x 10 ^ -3 Ka2 6.2 x 10 ^-8 Ka3 4.2 x 10 ^-13

Solid carbon can react with gaseous water to form carbon monoxide gas and hydrogen gas. The equilibrium constant for the reaction at 700.0 K is Kp=1.60×10−3If a 1.55-L reaction vessel initially contains 143 mbar of water at 700.0 K in contact with excess solid carbon, find the percent by mass of hydrogen gas of the gaseous reaction mixture at equilibrium.

1.) a key reaction in glycolysis is the isomerization of dihydroxyacetone into gylceraldehyde-3-phosphate. dhap<> G-3-P Delta G = 7.5 kj/mol

a.) whis is favored in this equilibrium, DHAP OR G-3-P?

B.) Calculate the equilibrium constant for the reaction at 25 degrees C.

C.) in the cell depletion of G-3-P makes the reaction proceed. what will delta G be if the temperature concentration of G-3-P is always kept 1/100 of the concentration of DHAP at a temp of 37 degrees C?

The atomic radius of an oxygen atom is 73 pm, and the ionic radius of the ion O2− is 140 pm. Explain the relative radii by estimating Zeff for each of these species.

Consider the titration of 171 mL of 0.961 M lactic acid, CH3CH9OH)COOH, Ka = 1.38E-4, with 1.203 M NaOH for the next three problems.

Problem #1

What is the pH of the solution when 83.33 mL of the 1.203 M NaOH are added to the 0.961 M lactic acid solution?

Problem #2

What is the pH of the solution at the equivalence point?

Problem #3

What is the pH of the solution when 178.9 mL of the 1.203 M NaOH has been added to the 0.961 M Lactic Acid solution?

Calculate the number of moles in 82.05 grams of Ca(NO3)2.
1 mole
2 moles
82.05 moles
0.50 moles

Question 3
Determine the number of grams in 0.5390 moles of calcium nitrate.
88.45 g
164.1 g
1 g
0.5390 g

Question 4
A sample of pure calcium nitrate has the same number of calcium cations as nitrate anions.
True
False

Question 5
A sample of calcium nitrate has twice as many nitrate anions as calcium cations.
True
False

Question 6
A sample of calcium nitrate that weighs 328.2 grams has
164.1 g of calcium
40.08 g Ca
80.16 g Ca
1 mole of calcium

Question 7
Place the following in order from the heaviest to the lightest.
- 1. 2. 3. 4. the mass of 1.2 moles of aluminum hydroxide
- 1. 2. 3. 4. the mass of one mole of calcium nitrate
- 1. 2. 3. 4. the mass of 1 mole of H2SO4
- 1. 2. 3. 4. the mass of 0.610 moles of calcium nitrate

Question 8
Is the formula weight of ammonium phosphate 149.33 g/mole? Pull all atomic weights from the periodic table with two decimal places to figure it out.
True
False

At 473 K, for the elementary reaction:

2NOCl(g)k1⇌k22NO(g)+Cl2(g)

k1=7.8×10−2L/mol⋅s and
k2=4.7×102L2/mol2⋅s

A sample of NOCl is placed in a container and heated to 473 K. When the system comes to equilibrium, [NOCl] is 0.24 mol/L.

Find the concentration of NO.

Find the concentration of Cl2

write the formular and names of FIVE examples of each of the following

(i) Nucleophiles

(ii) Electrophiles

(iii) Alkyl halide

(iv) leaving groups

Consider the chemical reaction and thermochemical information and initial partial pressures of the reaction components given below:



2H₂O(g) + 2Cl₂(g) ⇌ 4HCl(g) + O₂(g)

Determine ΔG (in kJ) for this reaction at 443.18 K. Assume ΔH°_f and S° do not vary as a function of temperature. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ).

he chromatogram below is for a solution containing a mixture of limonene and cymene, two naturally-occurring compounds found in lemon peel.

Limonene and cymene are present in an unknown proportion, so enough chlorobenzene is added to make its concentration in the solution equal to 0.0025 M.

Given that chlorobenzene has the lowest boiling point, and cymene has the highest boiling point, use the provided information to calculate the concentration of limonene in the mixture in moles per liter.

Complete combustion of 7.90 g of a hydrocarbon produced 24.2 g of CO2 and 11.6 g of H2O. What is the empirical formula for the hydrocarbon?