Write:

a) balanced equation

b) total ionic equation

c) net ionic equation

d) type of reaction

e)limiting reactant

1) Cu(s) + HNO3(aq) -> Cu(NO3)2 (aq)+ NO2(g) +H2O(l)

2) Cu(NO3)2(aq) + NaOH(aq) -> Cu(OH)2(s) + NaNO3

3) Cu(OH)2(s) -> CuO(s) +H2O

4) CuO(s) + H2SO4(aq) ->CuSO4(aq) +H2O(l)

5)CuSO4(aq) + Zn(s) -> Cu(s) +ZnSO4 (aq)

Calculate enthalpy for the following reaction Ca(s) + 1/2O2 + CO2 = CaCo3 Given the following reactions: Ca(s) + 1/2 O2 = CaO (s) H= -635.1 kj CaCo3 = CaO (s) + CO2 H= 178.3 kj

Consider a solution formed by mixing

50.0 mL of 0.100 M H₂SO₄,

30.0 mL of 0.1000 M HOCl,

25.0 mL of 0.200 M NaOH,

25.0 mL 0.100 M Ba(OH)₂, and

10.0 mL of 0.150 M KOH.

Calculte the pH of this solution.

K_a (HOCl) = 3.5 x 10^-8

What is the pH?

Chromatography explained in details highlighting important things to know for test.

Exothermic Vs. Endothermic Reaction

Reaction progress diagrams for single-step endothermic and exothermic reactions.

a. Devise a general statement about the relationship between Ea and the rate of a reaction. 


b. Describe the effect of temperature on the energy of collisions, and explain how this effect changes the rate of a reaction. 


c. State three things that resulted in an increase in the rate of the reaction. For each of the three things, explain at a molecular level what happens to cause the rate of the reaction to increase. 


A 12.9 mL solution of 0.100 mol L^-1 HOCl is titrated using 0.150 mol L^-1 NaOH.

What is the pH of the solution after 5.18 mL of the NaOH solution is added? Express your answer to 2 decimal places.

You have 5 attempts at this question.

Remember you can find K_A and/or K_B values in your textbook in chapter 15.

A saturated solution of barium fluoride, BaF2, was prepared by dissolving solid BaF2 in water. The concentration of Ba2+ ion in the solution was found to be 7.52

Compare and contrast the different types of chemical bonds and define the terms chemical bond, covalent bond (including polar and nonpolar), ionic bond, and hydrogen bond.

Balance each reaction, determine if they are ion-exchange, redox, or acid-base, and determine the direction of the reaction and if they are reverisble or irreversible and explain why.

NH₄ NO(s) – N(g) + H₂(g)

N₂ (g) + O₂ (g) – NO (g)

N₂ (g) + H₂ (g) – NH₃ (g)

H₂O (g) - O₂ (g) + H₂ (g)

CaCO₃ (s) – CaO (s) + CO₂ (g)

Cl₂ (g) + H₂O (l) – HCl (aq) + HClO (aq)

NH₄ (s) – NH₃ (g) + HCl (g)

Fe (s) + H₂SO₄ (aq) – FeSO₄ (aq) + H₂ (g)

CO₂ (g) + H₂O (l) – H₂CO₃ (aq)

Mg (s) + H₂O (l) – Mg(OH)₂ (aq) + H₂ (g)

CH₃-COOH (aq) + H₂O (l) - CH₃-COO^- (aq) + H₃O⁺(aq)

Write the formula of the coordination compound pentacarbonyliron(0)

Write a systematic name for Li₂[CoF₆].

Write a systematic name for [RuCl₂(bipy)₂].

Write a systematic name for [Co(NH₃)₃Cl₃].

9.) As mentioned below, you are required to design your own procedure for determining the heat of dissolution of your chosen salt with a coffee cup calorimeter. Answer the following questions and consider them in designing this procedure:

     a.) When you find your initial temperature T_i, should you take one measurement from the thermometer as soon as you place it in the water in the calorimeter? Why or why not? If not, what should you do instead?

     b.) Do you expect the temperature of the water in the calorimeter to rise, fall, or stay the same after you add your salt? If the temperature will change, will it continue to change indefinitely or not?

     c.) How will you know your dissolved salt solution has reached it's maximum or minimum temperature, i.e. what will you observe in your data to indicate this has happened?

     d.) Should you repeat your experiment? Why or why not? If so, what could you change from trial to trial? Give two possible suggestions, and determine which one you should change (as well as which one you should not!) in any subsequent trials you decide to perform.

*Information previously calculated is below*

1. Calculate the amount of heat (q) produced by the combustion of 4.05 g CH₄ (ΔH_comb = -890.4 kJ).

225.38 kj

2. Consider that the 4.05 g methane is burned and all of the heat from this combustion is absorbed by 1.0 kg of 20 °C water (use 4.18 g^-1 ºC^-1 for the specific heat of the water). What would be the final temperature of the water?

73.8°C

Estimate the pH of the resulting solution prepared by mixing 1.0 mole of solid disodium phosphate and 1.25 mole of hydrochloric acid. The pKas of phosphoric acid are 2.1,7.2,12.4. The answer is 2.1<pH<7.2. Please explain.

0.5 mole of a monatomic ideal gas is loaded into a cylinder and contained by a frictionless piston. The piston is set so that there is an initial volume of 2L. The gas in the cylinder is at a temperature of 298K. The gas is allowed to expand adiabatically against 1 atm of pressure. Calculate V/n initial, q per mole, w per mole, delta U per mole, delta S per mole and delta H per mole. What is the final temperature of the gas in Kelvin and Celcius?

1. What is natural radioactivity? Speak to the different types of radiation that an unstable nucleus may emit, and the different types of radiation involved.
2. Why is it important to be able to write a balanced nuclear equation for radioactive decay? Go into some of the specifics of what is involved in writing an equation.
3. What is a “half-life” and why is it important to know the half-life of a radioisotope? List a few applications of how scientists make use of having this knowledge. Why would it be so important to know the half-lives of radioisotopes when it comes to medical applications?
4. Briefly describe how we can make use our knowledge of radioactivity in medicine. Speak about the characteristics of the radioisotopes used in these types of applications. What might they have in common? What process(es) do we use to detect these radioisotopes?