Dale. 1 01 1 g Section:-S-Grade: Record all values with the correct number of si

Question

Dale. 1 01 1 g Section:-S-Grade: Record all values with the correct number of significant figures and units. Place all answers on the line next to the question. Show calculations for any numerical answers See any 102 TA in the help office before your prelab is dueif you have any questions. Your answer must be completely correct to get any credit for the answer, no partial credit. For the following redox reaction: Use the following chemicals to complete the questions. 1) What are the oxidation numbers for the Mn and Fe on the reactant side of the equation? MnCh (aq) + 2Fe(s)->2FeCl2(aq) +Mn(s) Fe 2) Identify the oxidizing agent in the equation. 3) Write the half-reaction associated with the reduction. 4) How many electrons are transferred in the reaction? 5) Calculate the molar mass of the MnCl4. 6) Calculate the mass percent of the cation in the MnCla

Explanation / Answer

MnCl4(aq) + 2 Fe(s) -------------------- 2 FeCl2(aq) + Mn(s)

1.

MnCl4

Oxidation state of Cl= -1

Sum of the oxidation states of all the atoms in a compound is equal to zero.

x + 4(-1) = 0

x=+4

so the oxidation state of Mn in MnCl4 = +4

Fe

oxdiation state of an atom of an element in native state is equal to zero.

In Fe , oxidation state of Fe = 0

2.

MnCl4(aq) + 2 Fe(s) -------------------- 2 FeCl2(aq) + Mn(s)

+4                      0                                   +2                   0

oxidation state of Mn is decreases from +4 to 0. so it undergoes reduction.Hence MnCl4 acts as Oxidising agent.

3.

MnCl4 ------------------- Mn

+4                                 0.

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