How much energy (in kilojoules) is released when 30.5g of ethanol vapor at 97.5?C is cooled to -16.5?C? Ethanol has mp = -114.5 ?C, bp = 78.4 ?C, ?Hvap = 38.56 kJ/mol and ?Hfusion = 4.60 kJ/mol. The molar heat capacity is 113 J/(K?mol) for the liquid and 65.7 J/(K?mol) for the vapor.

250 gallons of water (at 25 degrees Celsius and 1 atmospheric pressure) are boiled to power a steam engine. The heat source to boil the water is the combustion of methanol according the the reaction below. 2 CH3OH (liters) + 3 O2 (grams) −→ 2 CO2 (grams) + 4 H2O (liters) Using the enthalpy of the combustion of methanol (at 25 degrees Celsius and 1 atmospheric pressure), how many liters of methanol are required to boil the 250 gallons of water?

6. What is an addition reaction?


a. What type of starting materials are used for addition reactions? (functional group)


b. What type of reagents are used for addition reactions?

1) Glucose has molecular formula C6H12O6.

a) Draw the three distinct forms of glucose that exist in equilibrium in solution.

b) What is the term used to describe the inter-conversion of the three forms of glucose?

This is one question asked on my tutorial with no pictures etc. I'm at an absolute loss if you can help. Thank you!

Ionization energy is the energy needed to eject an electron from an atom or ion. Calculate the ionization energy, IE, of the one-electron ion Be3 . The electron starts in the lowest energy level, n=1.

Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) F2(g)+2e−→2F−(aq) +2.87 O2(g)+4H+(aq)+4e−→2H2O(l) +1.23 Br2(l)+2e−→2Br−(aq) +1.07 Ag++e−→Ag(s) +0.80 2H2O(l)+2e−→H2(g)+2OH−(aq) −0.83 Na+(aq)+e−→Na(s) −2.71 What is produced at each electrode in the electrolysis of an aqueous solution of both NaBr and AgF? Drag the appropriate items to their respective bins. Na(s) H2(g) F2(g) O2(g) Ag(s) Br2(l)

A 25.0mL of 0.152M H2SO4 was reacted with 20.0mL of 0.410 M NaOH.
Calculate the concentration of the salt that is formed during the reaction as well as the concentrations of H2SO4 and NaOH that remain in solution.

what is the purpose of a sandmeyer reaction (to get 4-chlorotoluene )

Predict a likely mode of decay for each of the following unstable nuclides.

Rh-92: beta decay or positron emission

Ga-60: beta decay or positron emission

S-27: beta decay or positron emission

Give 5 manifestations of the kinetic molecular theory or of gas laws in your every day life. For example, why does the low tire pressure warning light in your car turn on when the temperature cools dramatically? (DON'T answer that question, it's just an example lol). Thanks!!! I'll give the best answer the points.

I need to find the total and net ionic equations for the following reactions:

Thank you so extremely much in advance.

HCl (aq) + Al (s)

Fe(s) + HCl (aq)

Mg(s) + HCl (aq)

Zn(s) + HCl (aq)

Fe (s) + H2SO4 (aq)

Mg (s) + H2SO4 (aq)

Zn(s) + H2SO4 (aq)

Copper II Nitrate (aq) + Zinc(s)

At 1000 K, the value of K_c = 0.032 for the reaction:

C_(s) + H₂O_(g) ⟺ CO_(g) + H_2(g)

Calculate the equilibrium concentrations of H₂O, CO, and H₂ in a reaction mixture obtained by heating 6.05 mol of (H₂O) steam and excess of solid carbon in a 5.90 L container.

You can purchase nitric acid in a concentrated form that is 70.3% HNO(3) by mass and has a density of 1.41 g/mL. Describe exactly how to prepare 1.15 L of 0.100 M HNO(3) from the concentrated solution.

Please explain thoroughly.

A sample of mixture of FeSO4.(NH4)2So4.6H2O and inert material is dissolved in water, and the Fe is oxidized with bromine water. The excess Br2 is boiled out and NH4OH is added to precipitate the Fe(III). This precipitate, after ignition, weighs 0.160 g. Calculate a) the volume of the NH4OH (specific gravity 0.960, containing 10.0% Nh3 by weight) theoretically required in the above preecipitaion? b) The volume of 0.100 N BaCl2 solution required to precipitate the sulfate from the filtrate of the NH4OH precipitation.

At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3.

H2(g) + I2 (g) ---> 2 HI (g)

Kc= 53.3

At this temperature, 0.600 mol of H2 and 0.600 mol of I 2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?