Classify each of the following redox reactions as a combination, decomposition,
ID: 892195 • Letter: C
Question
Classify each of the following redox reactions as a combination, decomposition, or displacement reaction, give a balanced molecular equation for each, as well as total and net ionic equations for parts (b) and (c), and identify the oxidizing and reducing agents. (Type your answer using the format H2O for H2O and (NH4)2CO3 for (NH4)2CO3. Do not include state symbols in the answers. Use the lowest possible coefficients. Enter 0 if necessary. Do not leave any box blank.)
1) combination
2)decomposition
3) displacement
- molecular equation
1) combination
2) decomposition
3) displacement
1) combination
2) decomposition
3) displacement
Explanation / Answer
Answer – a) We are given the reaction and in this reaction there are two reacts reacted and formed one product, means two reactants combine in to each other and formed one product, so this is combination reaction. So answer is 1) combination
Now we need to balance to balance the molecular equation
--------- N2(g) + --------- O2(g) ---->------- NO(g)
In this reaction in the reactant side there are 2 N and 2 O and in product side there is 1 N and 1O , so we need 2 N and 2 O in the product side also, so balanced molecular reaction –
1 N2(g) + 1 O2(g) ----> 2 NO(g)
We know the reducing agent means the species which gets self-oxidized and force to other getting reduced. The oxidized compound act as reducing agent and reduction acts as oxidizing agent.
So in this reaction N2 and O2 both has 0 oxidation state and in the product there is +2 for N and -2 for O, so reducing agent is N2 and oxidizing agent is O2
b) In this given reaction there is replace the one atom from another atom. In reactant I gets replaced Cl, so this is the displacement reaction, answer is 3) displacement
Molecular reaction – In this given reaction in the reactant side 1 Cs, 1 I and 2 Cl and in product side there are 1 Cs, 2 I and 1 Cl, so we need to put 2 Cl in product side also
So reaction is -
---------- CsI(aq) + --------- Cl2(aq) ----> 2 CsCl(aq)) + -------- I2(aq)
Now we need 2 Cs in the reactant also, so reaction –
2 CsI(aq) + 1 Cl2(aq) ----> 2 CsCl(aq)) + 1 I2(aq)
Reducing agent – CsI
Oxidizing agent – Cl2
total ionic equation
2 Cs+(aq) + 2 I -(aq) + 1 Cl2(aq) ----> 2 Cs+(aq) + 2 Cl -(aq) + 1 I2(aq)
net ionic equation – In the net ionic reaction the ions which are present from both side gets cancel out -
2 I -(aq) + 1 Cl2(aq) ----> 2 Cl -(aq) + 1 I2(aq)
c) This one also displacement reaction, Ni gets replaced by the Cr, so answer is
3) displacement
Molecular equation -
1 Ni(NO3)2(aq) + 1 Cr(s) ----> 1 Ni(s) + 1 Cr(NO3)3(aq)
Reducing agent - Cr
Oxidizing agent – Ni(NO3)2
Total ionic equation -
1 Ni2+(aq) + 1 NO3-(aq) + 1 Cr(s) ----> 1 Ni(s) + 1 Cr3+(aq) + 1 NO3-(aq)
Net ionic equation-
1 Ni2+(aq) + 1 Cr(s) ----> 1 Ni(s) + 1 Cr3+(aq) + 1 NO3-(aq)