(a)
Interpretation:
The oxidation states to all the elements in the given reaction should be assigned along with identify the reactant which is oxidized and reduced and also identify the oxidizing agent and reducing agent in the given reaction.
Concept Introduction :
A redox reaction is a
Oxidation state or oxidation number of an atom is defined as the positive or the negative charge that an atom would possess if it is present as ions in the given compound. In such type of reaction, the oxidation state of the atom undergoing oxidation will increase which depends upon the number of electrons lost by a particular atom.
Reduction of a chemical species refers to the gain of electrons by the chemical species which results in decrease in oxidation state of that atom.
A reducing agent is one which loses its electrons for the reduction of other chemical species which are undergoing redox reactions. In other words we can say that a reducing agent in a chemical reaction is the species which itself gets oxidized by loss of its electrons.
On the other hand an oxidizing agent is a chemical species which has the ability to oxidize other substances which are present in a chemical reaction. It acts by gaining electrons in a chemical reaction, thus itself gets reduced.
(b)
Interpretation:
The oxidation states to all the elements in the given reaction should be assigned and identify the reactant which is oxidized and reduced and also identify the oxidizing agent and reducing agent in the given reaction.
Concept Introduction :
A redox reaction is a chemical reaction in which oxidation and reduction reactions takes place simultaneously. In such type of reaction one of the chemical species is getting oxidized while the other species gets reduced at the same time.
Oxidation state or oxidation number of an atom is defined as the positive or the negative charge that an atom would possess if it is present as ions in the given compound. In such type of reaction, the oxidation state of the atom undergoing oxidation will increase which depends upon the number of electrons lost by a particular atom.
Reduction of a chemical species refers to the gain of electrons by the chemical species which results in decrease in oxidation state of that atom.
A reducing agent is one which loses its electrons for the reduction of other chemical species which are undergoing redox reactions. In other words we can say that a reducing agent in a chemical reaction is the species which itself gets oxidized by loss of its electrons.
On the other hand an oxidizing agent is a chemical species which has the ability to oxidize other substances which are present in a chemical reaction. It acts by gaining electrons in a chemical reaction, thus itself gets reduced.
(c)
Interpretation:
The oxidation states to all the elements in the given reaction should be assigned and identify the reactant which is oxidized and reduced and also identify the oxidizing agent and reducing agent in the given reaction.
Concept Introduction :
A redox reaction is a chemical reaction in which oxidation and reduction reactions takes place simultaneously. In such type of reaction one of the chemical species is getting oxidized while the other species gets reduced at the same time.
Oxidation state or oxidation number of an atom is defined as the positive or the negative charge that an atom would possess if it is present as ions in the given compound. In such type of reaction, the oxidation state of the atom undergoing oxidation will increase which depends upon the number of electrons lost by a particular atom.
Reduction of a chemical species refers to the gain of electrons by the chemical species which results in decrease in oxidation state of that atom.
A reducing agent is one which loses its electrons for the reduction of other chemical species which are undergoing redox reactions. In other words we can say that a reducing agent in a chemical reaction is the species which itself gets oxidized by loss of its electrons.
On the other hand an oxidizing agent is a chemical species which has the ability to oxidize other substances which are present in a chemical reaction. It acts by gaining electrons in a chemical reaction, thus itself gets reduced.
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- Question 16 of 40 Balance the following chemical equation (if necessary): C3H,O2(g) + O2(g) → H2O(g) + CO2(g) H2O (g) + CO2 (g) 3C2 2- Reset 1. 2. 4 6. 8. 9. ) (s) (1) (g) (aq) LO 3.arrow_forward(7.1a) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. a) Cu(s) + NO3 (aq) - Cu*2(aq) + NO2(g) + NO29) Analysis: Oxidation-Half reation: Balancing atoms & charges: Cu(s) Cu*2, (aq) e Reduction-Half reation: Balancing O & H and charges: H* + NO3 (aq) e NO2(g) + 1 H20 Balancing electrons lost & gained and balancing the equation: Cu(s) NO3 (aq) + H* - Cu*(aq) NO2(g) H20arrow_forwardOnly 1 to 10arrow_forward
- Complete the following equations by writing the formula(s) of the product(s) and balancing the equation with coefficients. Use the type of reaction to aid in determining the products. 6. 7. 8. 9. Balanced Equation 10. Zn + FeCl3 + 12. C3H8 + HgO→ 13. Al + H₂SO4 → AgNO3 → 0₂ Cl₂ → Balanced Equation 11. Iron and oxygen react to form iron (III) oxide. afe +302 afe 203 Type of Reaction Single Replacement Write the balanced chemical equation for the following chemical reactions. Include the correct formulas for all reactants and products and balance with coefficients. Identify the type of reaction in the right column. Double Replacement Combustions Decomposition Combination Silver nitrate and magnesium chloride react to form magnesium nitrate and silver chloride. 2Aguo3 + MgCl₂ → 2 Agcl + ing [Nosta double displacement Type of Reaction Compustion Aluminum reacts with copper (II) sulfate to form aluminum sulfate and copper solid. 3 cu 50₂ +2A1-3 Cu +3504 +2A¹a (564)3 single displacment 10arrow_forwardAmmonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor. The following reaction takes place (at a certain temperature) as follows: 4 NH,(g) + 302(g) - 2 N2(g) + 6 H,O(g) 2.1 In the reaction above, identify which reactant is oxidized and which is reduced NH, O2 2.2 An industrial chemist studying this reaction fills a 500. mL flask with 1.3 atm of ammonia gas and 1.2 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of nitrogen gas to be 0.33 atm. Calculate the pressure equilibrium constant for this reaction. You must fill out the ICEE table below for full credit. Round your answer to 2 significant digits. Make sure to box your final answer for K,. If you need more space to show your work, please use the backside of this page 4 NH3(g) + 30,(g) 2 N2(g) + 6 H,0(g) Initial pressure Change Expression Equilibrium pressure K, = %3Darrow_forwardFor cach of the following compounds, give the oxidation state of each element in the compound. 1. CoO b. HCIO NACIO C. Fe(10.) d. H,SO For the balanced chemical equation shown below, calculate the oxidation states of all the reactants and products. Identify the elements that are oxidized and reduced, and identify the oxidizers and reducers. How many electrons were transferred during the course of the reaction? CO:(g) 2F:(g) → CF(g) Ox(g)arrow_forward
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