2) Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O2 (g) → 2Al2O3 (s) In a particular experiment, 5.0 g of Al reacts with 4.0 g of O2.

a) What is the limiting reactant in this reaction?

b) What is the theorectical yield of Al2O3?

c) How much of the excess reactant is left?

A 65.0 mL sample of 1.0 M NaOH is mixed with 48.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 24.4°C. After adding the NaOH solution to the coffee cup, the mixed solutions are stirred until reaction is complete. Assume that the density of the mixed solutions is 1.0 g/mL, that the specific heat of the mixed solutions is 4.18 J/(g •°C), and that no heat is lost to the surroundings. The ΔΗrxn for the neutralization of NaOH with H2SO4 is –114 kJ/mol H2SO4.

What is the maximum measured temperature in the Styrofoam cup? ---------

Also, 35.985 is incorrect as they mention at the site, "H₂SO₄ is not the limiting reagent. Remember to consider the stoichiometry of the balanced equation for the reaction".

Acetylene, C₂H₂ (boiling point = –84°C), is produced by the reaction of solid calcium carbide, CaC₂, and liquid water. Calcium hydroxide solution is the other product of the reaction. 127 kJ of energy is transferred to the atmosphere per mole of acetylene reacted. What mass of calcium carbide in kilograms and volume of water in gallons are needed to produce 125 cubic feet of acetylene at 17°C and 1.0 bar? What quantity of energy in megajoules will be transferred in the process?

Reaction 1: Cu(s) + AgNO3 (aq) = CuNO3 (aq) + Ag (s)

Reaction 2: Cu (s) +AgNO3 (aq) = Cu(NO3)2 (aq) + Ag (s)

Part 1: Write the balanced net ionic equations for both of the above reactions.

Assume that excess silver nitrate is available when answering the remaining questions.

Part 2: Calculate the theoretical grams of silver metal that could form from 2.568g of copper wire based upon reaction 1. (Be sure the reaction is properly balanced.)

Part 3: Calculate the theoretical grams of silver metal that could form from 2.568g of copper wire based upon reaction 2. (Be sure the reaction is properly balanced.)

Part 4: Calculate the percent yield of silver produced according to each reaction if a student isolates 8.021g of Ag once the entire 2.568g of copper wire has been consumed. Based upon these yields, which is the most likely reeaction to have occured? Explain your answer.

Calculate ?H^o,?S⁰,?G⁰ ( 25.0^oC)for the formation of sulfur trioxide from oxygen gas and sulfur dioxide ;

Wtite balance equation and show all units, substances in your equation.

a) Which of the following reactions occur when (E,Z,E)- octa-2,4,6-triene is heated? Circle your choice:

- Diels-Alder

-Cycloaddition

- Cope rearrangement

-Electrocyclic

-Sigmatropic

b) Sketch the MAJOR product that is formed when (E,Z,E)-octa-2,4,6-triene is heated. Be sure clearly show features such as the correct regio- and stereochemistry.

Sort the following reactions or processes based on whether they use energy from adenosine triphosphate (ATP), or produce energy to store as ATP. Drag the appropriate items to their respective bins. anabolic reaction, catabolic reaction,molecule transport and oxidation of fats. energy used or energy stored

Complete and balance the following equation:

S(s)+HNO3(aq)→H2SO3(aq)+N2O(g)(acidic solution)

Express your answer as a net chemical equation including phases.

Complete and balance the following equation:

BrO3−(aq)+N2H4(aq)→Br2(l)+N2(g)(acidic solution)

Express your answer as a net chemical equation including phases.

Complete and balance the following equation:

H2O2(aq)+ClO2(aq)→ClO2−(aq)+O2(g)(basic solution)

Determine the pH of a 0.046 M iodous acid (HIO2) solution. Iodous acid is a weak acid (Ka = 3.2 ✕ 10−5 M).

Calculate [OH ^-] and pH for each of the following solutions.



(a) 0.0043 M KOH

(b) 0.0341 g of CsOH in 540.0 mL of solution

(c) 28.1 mL of 0.00187 M Ca(OH)₂ diluted to 800 mL

(d) A solution formed by mixing 71.0 mL of 0.000480 M Ca(OH)₂ with 24.0 mL of 1.3 x 10^-3 M KOH

How do you find the lattice energy of ionic compounds?

1. a) What is the net ionic equation for ZnSO₄ + H₂O?

b) Is the solution acidic or basic?

c) Which ion, Zn²⁺ or SO₄^2-, is causing the observed acidity or basicity?

2. What is the net ionic equation for Na₂CO₃ + H₂O?

3. What is the net ionic equation for NaHSO₄ + H₂O?

a) How many grams of hydrogen gas (H2) is produced by the decomposition of 43.7g of ammonia gas (NH3)?

b) If 12.0 moles of H2 were produced, how many grams of NH3 was decomposed?

c) If 12.0 moles of H2 were produced, how many moles of N2 were produced?

2. Describe how you would prepare 100ml of 0.08 M sulfuric acid [H2SO4] from an 18 M concentrated sulfuric acid stock solution.

3. Describe how you would prepare 50 ml of 0.2 M potassium iodate [KIO3] dissolved in the 0.08 M sulfuric acid [H2SO4] that you have prepared above.

4. Describe how you would prepare 25 ml of 3.6 M hydrogen peroxide [h2O2] from a 30% (w/w) stock H2O2 solution (

5. Describe how you would prepare 50 ml of a 3% (w/v) soluble starch solution in water.

Molecular weights:

Malonic acid: 104.6

Manganese sulfate: 169.01

Potassium iodate: 214

Hydrogen peroxide: 34.01

1). Why do some oxygen containing hydrocarbons form hydrogen bonds and others do not?

2). A functional group R would attatch itself to which carbon of an n-propyl group?