The properties of alkenes and alkynes related to boiling, melting, polarity and solubility

A buffer composed of 0.50 mol acetic acid (HC₂H₃O₂) and 0.50 mol sodium acetate (Na⁺C₂H₃O₂^-) is diluted to a volume of 1.0 liter. The pH of the buffer is 4.74. How many moles of NaOH must be added to the buffer to raise its pH to 5.74?

4.) Consider the titration of 100.0 mL of 0.016 M HOCl (Ka=3.5×10−8) with 0.0400 M NaOH.

Part A

How many milliliters of 0.0400 M NaOH are required to reach the equivalence point?

Part B

Calculate the pH after the addition of 10.0 mL of 0.0400 M NaOH.

Part C

Calculate the pH halfway to the equivalence point .

Part D

Calculate the pH at the equivalence point.

The following table provides some information on carbon dioxide solubility in water.

Part A

What is the Henry's law constant for CO2 at 20∘C?

Express your answer in mol L−1 bar−1 to four decimal places.

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Part B

What pressure is required to achieve a CO2 concentration of 0.0980 mol L−1 at 20∘C?

Express your answer to three significant figures and include the appropriate units.

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Part C

At 1.01 bar, how many moles of CO2 are released by raising the temperature of 1 litre of water from 20∘C to 25∘C?

Express your answer to four decimal places and include the appropriate units.

there are 2 kinds of carbonyl acceptor structures in addition to benzoate esters that can be used in the reaction with phenylmagnesium bromide in order to produce triphenylmethanol. Also they react with a different number of equivalents of the Grignard Reagent. What are the carbonyl acceptors? please draw structure

If 155 mL of wet H2 is collected over water at 24 ∘C and a barometric pressure of 739 torr , how many grams of Zn have been consumed? (The vapor pressure of water is 22.38 torr.)

I have a couple questions the first one is:

1. Combine equations 1,2,3 to obtain equation 4. Then provide an equation for calculating the heat of reaction in kJ/mol.

Equation 1: MgO(s)+2HCl(aq)--->MgCl2(aq)+H2O(l)

Equation 2: Mg(s)+2HCl(aq)---->MgCl2(aq)+H2(g)

Equation 3: H2(g)+1/2O2(g)---->H2O(l)

2. Use Hess's Law to calculate the heat of reaction for the decompostion of methanol:

2CH3OH(l)--->2CH4(g)+O2(g)      Change Heat of reaction =?

Using this information:

H2O(g)--->H2(g)+1/2O2(g)            Change Heat= +241.82 kJ

CH4(g)+H2O(g)---->CO(g)+3H2(g) Change Heat = +206.10 kJ

2H2(g)+CO(g)---->CH3OH(l) Change Heat = -128.33 kJ

Maybe my assignment is poorly worded but I am confused as what to do, thank you for any help.

Be sure to answer all parts. Consider the reaction N2(g) + 3H2(g) → 2NH3(g)

ΔH o rxn = −92.6 kJ/mol

If 4.0 moles of N2 react with 12.0 moles of H2 to form NH3, calculate the work done (in joules) against a pressure of 1.0 atm at 25°C.

?w = (Enter your answer in scientific notation.)

What is ΔU for this reaction? Assume the reaction goes to completion. ΔU = kJ

Calculate the cell potential, at 25^oC, for the reaction

3 Zn(s) + 2 Cr⁺³(aq)[0.010 M] --> 3 Zn⁺²(aq)[0.020 M] + 2 Cr(s)

given,

Cr⁺³(aq) + 3e^- --> Cr(s) . . . . . . . E^o= -0.74 V

Zn⁺²(aq) + 2e^- --> Zn(s) . . . . . . E^o = -0.76 V

Question options:

Consider the hydroboration of 1-pentene. Predict the major outcome of this reaction through a transition state analysis and construct a reaction coordinate diagram to justify your answer. Note: the oxidation step after hydroboration does not have any impact on regioselectivity.

Each of the solvents listed below are used in experiments in this text to extract organic compounds from aqueous solutions.

(i)Methylene chloride

(ii)pentane

(iii)Toluene

(iv)Diethyl ether

Will the organic phase be the upper or lower layer when each of these solvents is mixed with water? Explain your an- swer for each case. (b) If you placed an ice cube in each of the solvents i–iv listed above in (a), would you expect an ice cube placed in each to float? Explain your answer for each case

You wash dishes for a chemistry laboratory to make extra money for laundry. You earn 12 dollars/hour, and each shift lasts 75 minutes. Your laundry requires 12 quarters/load.

Part A

How many shifts must you work if you wish to wash 10 loads of laundry?

Part B

How many loads of laundry can you wash if you work 3 shifts?

Part C

How many loads of laundry will each shift pay for if the cost per load rises to 16 quarters?

a 0.490 g sample of a compound is heated through the successive evolution of the following gases, all at 1.00atm pressure: 280 ml of h2o vapor at 182ºC, 112ml of ammonia vapor at 273ºC, 0.0225g ofwater at 400ºC and 0.200g of SO3 at 700ºC, At the end of the heating, 0.090 g of FeO remains. Deduce the empirical formula for the compound

A gas chromatogram of the organic components of a sample of beer using a column that separates compounds on the basis of their relative boiling points provides a GC trace with several peaks. Two of the smaller peaks, with retention times of 9.56 and 16.23 minutes, are believed to be ethyl acetate and ethyl butyrate, respectively.

a. From the above information, which component of the sample, ethyl acetate or ethyl butyrate, elutes faster? What are the reported boiling points of these two substances?

b. What GC experiment(s) could you perform to confirm the identity of the peaks at 9.56 and 16.23 minutes?

c. Suggest two ways in which you could adjust the conditions of the experiment so as to reduce the retention time for all components in the sample.

How much heat energy is required to convert 55.4 g of solid iron at 21 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/g·°C.