What are the basic differences between SNAr reaction with SN1 and SN2 reactions?

Part A Suppose that a fully charged lead-acid battery contains 1.50 L of 5.00 M H2SO4. What will be the concentration of H2SO4 in the battery after 3.80 A of current is drawn from the battery for 7.00 hours ? Express your answer with the appropriate units.

Phosphoric Acid, H3PO4(aq) is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations(M) of all species in a 0.300 M phosphoric acid solution.

pKa1= 2.16 pKa2=7.21 pKa3=12.32

[H3PO4]=

[H2PO4-]=

[HPO4^2-]=

[PO4^3-]

[H+]=

[OH-]=

pH=

A combustion reaction of a hydrocarbon is defined as the reaction of the compound into carbon dioxide and water.

CmHn(g) + (m+(1/4)n)O2(g) ---> mCO2 + (1/2)nH2O(l)

1. Demonstrate that this chemical reaction is balanced.

2a. From this definition, write down the chemical reaction for the combustion of cyclopropane, C3H6(g).

2b. The enthalpy of reaction for the combustion of cyclopropane (i.e., the reaction in 2a) is measured to be ΔH° rxn = −2091 kJ/mol in the standard state at 25° C. Find the standard state enthalpy of formation, ΔH° f , at 25° C for CO2(g) and H2O(l) in a chemistry textbook. Use this information to determine the enthalpy of formation for cyclopropane in the standard state at 25° C.

2c. Propene is an isomer of cyclopropane. At 1bar pressure and a temperature of 25° C, the enthalpy of formation for propene is +20.42 kJ mol-1 . Determine the enthalpy of reaction for the isomerization reaction:

cyclopropane (g) → propene (g) ,

at 1bar pressure and a temperature of 25° C.

A) What is the pH of a solution with a fluoride concentration of 0.272 M? The Kb for F- is 1.47 x 10^-11.

B) Calculate the pH value of of a 0.015 M solution of pyridine, C5H5N. The Kb of pyridine is 1.7 x 10^-9. Enter your values for a, b, and c for the quadratic equation along with the final answer.

2 reacts with the halogens (X2) according to the following reaction:
H2(g)+X2(g)?2HX(g)
where X2 can be Cl2, Br2, or I2.

Assuming deltaG^o for the reaction between hydrogen and Cl2 is -190.46 kJ calculate Kp for the reaction between hydrogen and Cl2.

How to solve: A solution of K2Cr2O7 is standardized against Fe(NH4)2(SO4)2 6H20. Exactly 0.625g of the iron salt are equivalent to 22.5 mL of the dichromate solution. A sample of unknown iron (II) is then titrated with the dichromate. Exactly 25.0 mL of the iron are equivalent to 18 mL of the K2Cr2O7 solution. Calculate the number of millimoles of iron per mL of unknown solution. The answer is 2.98 mg/mL

Calculate the [H3O+] and pH of each polyprotic acid solution.

Dissociation Constants for Acids at 25 ∘C

PART A

0.130 M H3C6H5O7 H3O+ =

PART B

0.130 M H3C6H5O7 pH =

What are the primary sources of error in an experiment where you are calculating the caloric content of food by using a calorimeter that could explain any differences between you data and the label infomation for the number of Calories per gram? (Hint: How do these sources of error relate to the assumption that Qlost=Qgained?)

Consider the reaction: C2H4(g) + H2(g) <-> C2H6(g). For this process, deltaH = -137.0 kj/mol and deltaS = -120.6 J/mol*K. Based on these data and assuming deltaH and deltaS are temperature independent, answer the following questions;

1) Does this reaction favor products or reactants at 25 degrees C?

2) At 25 degrees C, is the reaction driven(dominated) by the entropy or the enthalpy?

3) Would a decrease in temperaturefavor the reactants or the products?

4) At what temperature would the equilibrium constant (K) equal unity (=1.0)?

The answers should be 1:products, 2:enthalpy, 3:products and 4:???? but I don't know why! Explaination please and answer to #4.

Remember the expert uses the numbers in the problem rounded to the correct significant digits. The expert allows plus or minus 3% error in a calculation. So be careful when judging the expert's response. You may be using the correct approach, but have a minor math, substitution, or rounding error.

1) A sample of water in the vapor phase (no liquid present) in a flask of constant volume exerts a pressure of 450 mm Hg at 98 C. The flask is slowly cooled.

a). Assuming no condensation, use the Ideal Gas Law to calculate the pressure of the vapor at 87 C; at 72 C.

b) On the basis of your answers in a) and b), predict the pressure exerted by the water vapor in the flask at 87 C; at 72 C.

2) Consider two closed containers each partially filled with liquid water one at 87 C and the other at 72 C. Can the pressure of water vapor in the gas phase in either container ever exceed the equilibrium vapor pressure at the particular temperature? What is the vapor pressure for water at 87 C and at 72C?

3) Write a chemical equation describing the condensation process for N₂ and a chemical equation describing the freezing process for N₂. For each process discuss the change in enthalpy and entropy that occurs. For each process describe the conditions (in terms of temperature) that support a thermodynamically favorable change, and the conditions that do not support a thermodynamically favorable change.

4) The normal boiling point of methanol is 65.0 C and its Hvap = 37.4 kJ mol-1. Calculate the temperature at which methanol has a vapor pressure of 180.08 mmHg.

Twenty kg of a fuel consisting of 50% methane, 25% ethane and 25% propane (by mass) is compressed to 180 atm and 100 degrees C. What is the compressed volume using Kay’s rule?

A furnace is burning natural gas (90% by mol methane and the balance ethane) at 20 degrees C and 1 atm with 25% excess air at 150 degrees C and 1.1 atm. The product gases are at 600 degrees C and 1 atm. 95% of each fuel gas forms CO2 while the balance forms CO. a) What is the ratio of air supply volume to fuel volume? b) What is the composition of the product gas mixture on a mol% basis? c) What is the ratio of exhaust gas volume to fuel volume?

Find the pH and the volume (mL) of 0.487 M HNO3 needed to reach the equivalence point in the titration of 2.65 L of 0.0750 M pyridine (C5H5N)?