A chemist isolated 0.7886 g of isoamyl acetate from a reaction of 0.8235 g of isoamyl alcohol and 1.5 mL of acetic acid.

What is the percent yield for the reaction above?

4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)

A scientist adds 7.00 atm of NH₃(g) and 8.00 atm of O₂(g) to a 5.0 L container at 473 K. What will the pressure of H₂O(g) be if the reaction goes to completion? Assume that the temperature remains constant.

Select one:

a. 6.40 atm

b. 9.60 atm

c. 10.5 atm

d. 0.90 atm

e. 15.0 atm

Question 3: Draw the titration curve (pH versus mL of NaOH added) that would be obtained from the titration of 30 mL of a 0.10 M solution of an unknown triprotic acid, H3A (Ka1 = 1.26 x 10–3; Ka2 = 5.6 x 10–6; Ka3 = 3.32 x 10–10) with 0.10 M NaOH. Indicate the volume needed to reach the first, second, and third equivalence points and the pH at the half equivalence points for the three titration regions.

The heating value of combustible fuels is evaluated based on the quantities known as the higher heating value (HHV) and the lower heating value (LHV). The HHV has a higher absolute value and is obtained by assuming that the water formed in the combustion reaction is formed in the liquid state. The LHV has a lower absolute value and is obtained by assuming that the water formed in the combustion reaction is formed in the gaseous state. The LHV is therefore the sum of the HHV (which is negative) and the heat of vaporization of water for the number of moles of water formed in the reaction (which is positive). The table below lists the enthalpy of combustion (which is equivalent to the HHV) for several closely related hydrocarbons. Use the information in the table to answer the following questions.

Part A

Given the provided data, complete and balance the combustion equation for the combustion of butane, CH3CH2CH2CH3CH3CH2CH2CH3, using whole-number coefficients for CO2CO2 and H2OH2O, assuming liquid water forms:

CH3CH2CH2CH3(g)+O2(g)→     ––– +      –––CH3CH2CH2CH3(g)+O2(g)→     _ +      _

Express your answer as a balanced chemical equation using the smallest whole-number coefficients including phases.

View Available Hint(s)

Part B

The following table lists heat of formation values for select compounds:

Part C

Calculate ΔHΔH for the combustion of one mole of butane gas, C4H10C4H10, assuming H2O(l)H2O(l) is produced instead of H2O(g)H2O(g).

Express the change in enthalpy in kilojoules to five significant figures.

Part D

Calculate ΔHΔH for the combustion of one mole of butane gas, C4H10C4H10, assuming H2O(g)H2O(g) is produced instead of H2O(l)H2O(l).

Express the change in enthalpy in kilojoules to five significant figures.

Because of the toxicity of mercury compounds, mercury(I) chloride is used in antibacterial salves. The mercury(I) ion (Hg2 2+ ) consists of two bound Hg+ ions.

a. What is the chemical formula of mercury(I) chloride? (1 mark)

b. Calculate [Hg2 2+ ] in a saturated solution of mercury(I) chloride (Ksp = 1.5 x 10-18 ).

c. Seawater contains 0.03 kg of NaCl per litre. Using a suitable approximation, find [Hg2 2+ ] if the seawater is saturated with mercury(I) chloride.

d. How many grams of mercury(I) chloride are needed to saturate 4900 km3 of water (the volume of Lake Michigan)? e. How many grams of mercury(I) chloride are needed to saturate 4900 km3 of seawater?

Calculate the expected pH when 0.5 mL of 0.1 M HCL is added to 30.0 mL pure water. Do the same calculation when the same amount of HCl is added to 30.0 mL of your original .05M buffer. Compare the calculated pH to the actual measured pH.

My buffer has a pH of 5.09 and I used acetic acid which has a pKa of 4.76

2.
If you have 50 mL of .05M potassium phosphate buffer pH 7.0 and you added 2.0 mL of 0.1M HCl what would the final pH be? What would the pH be if 2.0 mL of 0.1M NaOH was added to the same amount of the original buffer?

12.0 L container of sulfur dioxide has a pressure of 285 Torr T -110oC. What mass of SO2 is present?

Which of the following compounds would produce a negative test for chromicacidand a positive test for 2,4-dinitrophenylhydrazine, be soluble in sulfuric acidand be insoluble in sodium bicarbonate: methyl m-nitrobenzoate, 2-pentanone, or 1-octanol? 


Draw (1S,3S)-3-methylcyclopentanol and explain your reasoning.

1. Propose a method to test the antioxidant activity (DPPH Scavenging method) of organic compounds. Write a detailed report about the protocol. Write the purpose, materials, calculations, methods, etc.

Acetic acid has a normal boiling point of 118 ∘C and a ΔHvap of 23.4 kJ/mol.What is the vapor pressure (in mmHg) of acetic acid at 40 ∘C?

how do you find bond angle measurement with a line bond structures

One mole of an ideal gas at 1.00 atm and 298K with C_{p,m=3.5R is put through the}

following cycle: a) (reversible) constant volume heating to twice its initial

temperature; b) reversible, adiabatic expansion back to its initial temperature;

c) reversible isothermal compression back to 1.00 atm. Calculate ΔS for each step and

overall. d) What is the change of entropy of the surroundings?

A chemistry graduate student is given 100.mL of a 1.50M diethylamine C2H52NH solution. Diethylamine is a weak base with =Kb×1.310−3. What mass of C2H52NH2Cl should the student dissolve in the C2H52NH solution to turn it into a buffer with pH =11.35? You may assume that the volume of the solution doesn't change when the C2H52NH2Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.