N₂ + 3H₂>>>2NH₃

Using the equation above, calculate how many grams of NH₃ you would have if you started with 2.37 g of N₂ and 2.37 g of H₂?

Calculate the value of Eocell for the following reaction: 2Co3+(aq) + 3Ca(s) --> 2Co(s) + 3Ca2+(aq) Co3+(aq) + 3e– --> Co(s) Eo = 1.54 V Ca2+(aq) + 2e– --> Ca(s) Eo = –2.87 V.

A. –1.33 V

B. +1.33 V

C. –4.41 V

D. –11.6 V

E. +4.41 V

Why do we use atomic absorption spectroscopy?

What equations are/can be used to describe the velocity profile for a turbulet flow in a pipe and how do you visualise the plot in excel?

Imagine that you are attempting to determine the concentration of an acid by titration with a solution of sodium hydroxide with a known concentration, using phenolphthalein as an indicator. For each of the following sources of error, indicate whether the calculated concentration of acid would be too high or too low.

i. An air bubble was present in the tip of the buret before beginning the titration but was absent at the end of the titration.

ii. You added too much base and went beyond the end point.

iii. Some of the acid splashed on to the sides of the flask and wasn’t titrated.

Describe the kinetic differences between an uncatalyzed second order chemical reaction and an enzyme catalyzed reaction.

Which statement is NOT correct?

A. You can increase entropy and still have a spontaneous reaction.

B. If there is a decrease in the energy of the system, the reaction is spontaneous.

C. Spontaneous reactions will tend to maximize entropy and minimize enthalpy at given temperature

D. Entropy can drive a reaction that is strongly endothermic

How long will it take to plate 1.25 grams of Copper metal from a solution of CuSO₄, if a current of 2.0 A is used? Assume 100% efficiency.

Part A

Which of the following ionic compounds is expected to have the highest lattice energy?

Part B

Which of the following atoms could form a fluoride compound (i.e. MF_n) in which M has an "expanded octet" (more than an octet on the centrat atom)?

Part C

Which of the elements below, when found in a covalently bonded compound, could have an incomplete octet (have less than a full octet of electrons) and still have a valid Lewis Structure?

21.83 mL of a Pb2 solution, containing excess Pb2 , was added to 10.75 mL of a 2,3-dimercapto-1-propanol (BAL) solution of unknown concentration, forming the 1:1 Pb2 –BAL complex. The excess Pb2 was titrated with 0.0141 M EDTA, requiring 8.86 mL to reach the equivalence point. Separately, 40.70 mL of the EDTA solution was required to titrate 31.00 mL of the Pb2 solution. Calculate the BAL concentration, in molarity, of the original 10.75-mL solution.

Classify the reaction Ca(OH)2 (aq) + H2CO3(aq) → CaCO3(s) + 2 H2O(l):
a. Acid-Base b. Precipitation c. Both d. Neither
Sodium phosphate reacts with calcium chloride. Write the balanced, net ionic equation, and then choose the coefficient associated with the calcium ion in that equation (choose 0 if not present):
a. 0 b. 1 c. 2 d. 3
Sulfuric acid reacts with barium hydroxide. Write the balanced, net ionic equation, and then choose the coefficient associated with the hydroxide ion in that equation (choose 0 if not present):
a. 0 b. 1 c. 2 d. 3
Sulfuric acid reacts with ammonia. Write the balanced, net ionic equation, and then choose the coefficient associated with the sulfate ion in that equation (choose 0 if not present):
a. 0 b. 1 c. 2 d. 3

Please show any work

what reaction type is

Cu²⁺ + OH^-   ---> Cu(OH)₂

CuSO₄ x 5H₂O ----> CuSO₄

CuSO₄ ------> CuSO₄ x 5H₂O

NH₄Cl -----> NH₃ + HCl

Reaction Type Options are:

1. Combination, Synthesis or Formation Reaction

2. Decomposition Reaction

3. Single Displacement or Single Replacement Reaction

4. Double Displacement or Double Replacement Reaction

Is the ionic compound CaCO3 soluble or insoluble, and does each of its ions tend to be soluble?

a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble

Is the ionic compound NaNO3 soluble or insoluble, and does each of its ions tend to be soluble?

a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble

Is the ionic compound AgBr soluble or insoluble, and does each of its ions tend to be soluble?

a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble

Is the ionic compound (NH4)3PO4 soluble or insoluble, and does each of its ions tend to be soluble?

a. Both ions soluble b. Both ions insoluble c. Ions differ; soluble d. Ions differ; insoluble

Classify the solution properties of 1.0 M acetic acid.

a. Strong electrolyte b. Weak electrolyte c. Non-electrolyte d. Pure liquid

Please Show Work

How can the Van Der Waals equation of state be used to determine whether a substance will be a solid, liquid or gas at a certain temperature and pressure?

Write a chemical reaction and a few words to explain why the pH of the formic acid buffer above goes up only tenths of a pH unit (from about 3.6 to about 3.7 pH units) when a few drops of 0.10 M NaOH solution are added to it, instead of going up much more to about pH=10. {Note that if the same amount of NaOH were added to 20 mL of 0.00025 M HCl (which also has pH=3.6), the pH would go up to about pH=10. Explain qualitatively – no calculation is needed.}