Question

In: Chemistry

H2SO4 + Mg Can someone show the steps in solving that REDOX reaction? Need to show...

H2SO4 + Mg

Can someone show the steps in solving that REDOX reaction?

Need to show balanced reaction, Complete Ionic equation

and the Half Ionic. What is the purpose of showing the half

Ionic? When solving Redox reactions do you always

need to show the half reactions? thanks much

Solutions

Expert Solution

Step 1. Write down the unbalanced equation ('skeleton equation') of the chemical reaction. All reactants and products must be known. For a better result write the reaction in ionic form.

Mg + H2SO4 → MgSO4 + H2

Step 2. Separate the redox reaction into half-reactions. A redox reaction is nothing but both oxidation and reduction reactions taking place simultaneously.

a) Assign oxidation numbers for each atom in the equation. Oxidation number (also called oxidation state) is a measure of the degree of oxidation of an atom in a substance (see: Rules for assigning oxidation numbers).

b) Identify and write out all redox couples in reaction. Identify which reactants are being oxidized (the oxidation number increases when it reacts) and which are being reduced (the oxidation number goes down).

When one member of the redox couple is oxygen with an oxidation state of -2 or hydrogen with an oxidation state of +1, it is best to replace it with a water molecule.

O: (Mg)

R: (H)

c) Combine these redox couples into two half-reactions: one for the oxidation, and one for the reduction. (see: Divide the redox reaction into two half-reactions).

O:   

R:   

Step 3. Balance the atoms in each half reaction. A chemical equation must have the same number of atoms of each element on both sides of the equation. Add appropriate coefficients (stoichiometric coefficients) in front of the chemical formulas. Never change a formula when balancing an equation. Balance each half reaction separately.

a) Balance all other atoms except hydrogen and oxygen. We can use any of the species that appear in the skeleton equations for this purpose. Keep in mind that reactants should be added only to the left side of the equation and products to the right.

O:  Mg + H2SO4 → MgSO4

R: H2O → H2

b) Balance the oxygen atoms. Check if there are the same numbers of oxygen atoms on the left and right side, if they aren't equilibrate these atoms by adding water molecules.

O: Mg + H2SO4 → MgSO4

R: H2O → H2 + H2O

c) Balance the hydrogen atoms. Check if there are the same numbers of hydrogen atoms on the left and right side, if they aren't equilibrate these atoms by adding protons (H+).

O:   Mg + H2SO4 → MgSO4 + 2H+

R:   H2O + 2H+ → H2 + H2O

Step 4. Balance the charge. To balance the charge, add electrons (e-) to the more positive side to equal the less positive side of the half-reaction. It doesn't matter what the charge is as long as it is the same on both sides.

O: Mg + H2SO4 → MgSO4 + 2H+ + 2e-

R: H2O + 2H+ + 2e- → H2 + H2O

Step 5. Make electron gain equivalent to electron lost. The electrons lost in the oxidation half-reaction must be equal the electrons gained in the reduction half-reaction. To make the two equal, multiply the coefficients of all species by integers producing the lowest common multiple between the half-reactions.

O: Mg + H2SO4 → MgSO4 + 2H+ + 2e- | *1

R:  H2O + 2H+ + 2e- → H2 + H2O | *1

O:  Mg + H2SO4 → MgSO4 + 2H+ + 2e-

R:  H2O + 2H+ + 2e- → H2 + H2O

Step 6. Add the half-reactions together. The two half-reactions can be combined just like two algebraic equations, with the arrow serving as the equals sign. Recombine the two half-reactions by adding all the reactants together on one side and all of the products together on the other side.

Mg + H2O + H2SO4 + 2H+ + 2e- → MgSO4 + H2 + 2H+ + H2O + 2e-

Step 7. Simplify the equation. The same species on opposite sides of the arrow can be canceled. Write the equation so that the coefficients are the smallest set of integers possible.

Mg + H2SO4 → MgSO4 + H2

Finally, always check to see that the equation is balanced. First, verify that the equation contains the same type and number of atoms on both sides of the equation.


Related Solutions

Balance the following redox reaction if it occurs in H2SO4. What are the coefficients in front...
Balance the following redox reaction if it occurs in H2SO4. What are the coefficients in front of H2O and Cr2(SO4)3 in the balanced reaction? C3H8O2(aq) + K2Cr2O7(aq) → C3H4O4(aq) + Cr2(SO4)3(aq) Can someone please explain everything step by step since how to determine oxidation numbers and half reactions?
Balance the redox reaction FeSO4 + H2SO4 + KMnO4 ---> Fe2(SO4)3 + K2SO + MnSO4 +...
Balance the redox reaction FeSO4 + H2SO4 + KMnO4 ---> Fe2(SO4)3 + K2SO + MnSO4 + H2O What is the coefficient of FeSO4 in the balanced equation? Please show work.
Can someone show me the steps of how to solve this? A program needs to access...
Can someone show me the steps of how to solve this? A program needs to access the following pages: 1, 2, 3, 4, 2, 1, 3, 2, 1, 4, 2, 3 There are 3 initially empty frames, how many page faults will there be respectively, if we use First-in-First-out, and Farthest-in-Future page replacement algorithms? A) 7 and 7 B) 7 and 6 --  Correct Answer   C) 6 and 6 D) 6 and 5
Can someone show me how to break this down by steps please and thank you. You...
Can someone show me how to break this down by steps please and thank you. You sell short 200 shares of a stock at $95 on a 60% initial margin requirement with a 30% maintenance margin. In 3 months, the stock is $79. What is your margin at this time? When would a margin call occur? If you cover your position when the stock is $79, what would be your HPR? Assume you did the same trade as before but...
without using excel can someone show me the steps to approach the following question Question 2...
without using excel can someone show me the steps to approach the following question Question 2 Rump Industries Ltd expects its new product will give it a significant first mover advantage in the market and that is expected to provide growth in earnings per share of 400% within the coming year, and 75% growth in each of the subsequent 3 years. After that time, it is expected competitors will have developed and brought to market similar products with the result...
Balance the following reactions in BASIC conditions. Show all steps. 1) Mg + NO3-1 ---> Mg...
Balance the following reactions in BASIC conditions. Show all steps. 1) Mg + NO3-1 ---> Mg +2 + N2 2) MnO4-1 + H2SO3 ---> Mn2+ + SO4-2 3) Cl-1 + MnO4-1---> ClO3-1 + MnO2 4) MnO4-(aq) + Fe2+(aq) ---> Mn2+(aq) + Fe3+(aq)
Show a balanced equation for the redox reaction for the oxidation of paranitrotoluene using chromic acid...
Show a balanced equation for the redox reaction for the oxidation of paranitrotoluene using chromic acid (H2CrO4) as the oxidizing agent. (Note that the oxidation of state of Cr goes from 6+ to 3+ and the toluene give up 3 H+'s) Calculate the theoretical yield and percentage yield of the acid from the reaction of OXIDATION OF AN ALKYL AROMATIC COMPOUND Procedure: Place 1.5 g of the para-nitrotoluene and 8 mL glacial acetic acid in a reflux flask.Pour 12 mL...
balance the redox reaction NO2- + MnO4- + H+ -------> NO3- + Mn2+ + H2O show...
balance the redox reaction NO2- + MnO4- + H+ -------> NO3- + Mn2+ + H2O show work please
1. a) Show the balanced half reactions and the total balanced reaction for the following redox...
1. a) Show the balanced half reactions and the total balanced reaction for the following redox reaction in acidic solution. RuO4 + H2SeO3 → Ru3+ + SeO42- b) Comment on whether you expect this reaction to be spontaneous. Show all of your work.b 2 (a) Use the Lattimer diagram for chlorine in basic conditions to determine the potential for reduction of ClO4- to Cl2 . (b) Write a balanced equation for this half reaction
PLEASE SHOW ME YOUR STEPS!! Consider the following unbalanced redox equations: a. I
PLEASE SHOW ME YOUR STEPS!! Consider the following unbalanced redox equations: a. I
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT