Complete and balance each equation. If no reaction occurs, write NOREACTION.

a) NaNO3(aq)+KCl(aq)?

b) NaCl(aq)+Hg2(C2H3O2)2(aq)?

c) (NH4)2S(aq)+SrCl2(aq)?

d) Al2(SO4)3(aq)+AgNO3(aq)?

Thanks

Part A What mass of calcium can be produced by this process if a current of 6300 A is applied for 39 h ? Assume that the electrolytic cell is 65 % efficient. Part A What mass of calcium can be produced by this process if a current of 6300 A is applied for 39 h ? Assume that the electrolytic cell is 65 % efficient. Part B What is the minimum voltage needed to cause the electrolysis?

Part B

How many minutes are needed to plate out 22.00 g Mg from molten MgCl2, using 3.00 A of current?

Calculate ΔH∘ in kilojoules for the reaction of acetylene (C2H2) (ΔH∘f=227.4kJ/mol) with O2 to yield carbon dioxide (CO2)(ΔH∘f=−393.5 kJ/mol) and H2O(g) (ΔH∘f=−241.8kJ/mol), a reaction which is supplied by the industrial gases industry for oxyacetylene gas welding and cutting due to the high temperature of the flame.

2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g)

Express your answer using one decimal place.

Johnny had a 50.0 mL sample of 0.4360 M NH₄NO₃ that he diluted with water to a total volume of 250.0 mL. He has to figure out what is the ammonium nitrate concentration in the resulting solution? Go to this link https://youtu.be/MG86IFZi_XM

a) what equation is used? And what 2 pieces of glassware are used – explain what for

Johnny has to make the 0.1510 M NaOH solution needed for his lab. If he uses a 100.00mL volumetric flask, how many grams of NaOH does he need

b) explain how you would make this solution (so you will need to know grams of NaOH)

Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor: 40.0 g NH₃ and 50.0 g O₂ are allowed to react according to the following equation:

4NH₃ + 5O₂ à 4NO + 6H₂O

4. What is the maximum number of grams of nitric oxide that can be produced in this experiment?

                     a. 50.0 g

                     b. 70.6 g                       

                     c. 37.5 g

                     d. 40.0 g

                     e. 58.6 g

A 130.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br.

A) What mass of HCl could this buffer neutralize before the pH fell below 9.00? ​answer to this was 0.088g

B) If the same volume of the buffer were 0.265 M in NH3 and 0.395 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?

A standard galvanic cell is constructed in which a Cd²⁺ | Cd half cell acts as the cathode. Which of the following statements are correct?

Hint: Refer to a table of standard reduction potentials.

(Choose all that apply.)

1. The anode compartment could be F₂|F^-.

2. The anode reaction could be Cr -> Cr³⁺ + 3e^-

3. Cd²⁺ is reduced at the cathode.

4. As the cell runs, anions will migrate from the Cd²⁺|Cd compartment to the other compartment.

5. The cathode reaction is Cd -> Cd²⁺ + 2e^-

In which of the following pairings of compounds are both members of the pair strong
electrolytes?

draw full sn1 mechanism for a reaction that includes 2-methyl-2-propanol, n-pentanol and hydrochloric acid as the reactants and 2-chloro-2-methylbutane and 1-chloropentane as products.

Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction

NH4HS(s)?NH3(g)+H2S(g)

This reaction has a Kp value of 0.120 at 25 ?C.


An empty 5.00-L flask is charged with 0.400g of pure H2S(g), at 25 ?C.

What is the initial pressure of H2S(g) in the flask?

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa. K_a (HCOOH) = 1.7x10^{-4 ? 3.4% is correct answer}

Calculate the pH at the equivalence point in titrating 0.110 M solutions of each of the following with 8.0×10−2 MNaOH. chlorous acid (HClO2) benzoic acid (C6H5COOH)