Q: 1. Identify the oxidation number of the specified element in each of the following entities: (f) N…
A: Since you have asked multiple parts we will solve the first three parts for you. If you want any…
Q: 3. Use the changes in oxidation numbers to identify which atoms are oxidized and which are reduced…
A:
Q: 3. Use the changes in oxidation numbers to identify which atoms are oxidized and which are reduced…
A:
Q: 4.45 Give the oxidation numbers for the underlined atoms in the following molecules and ions: (a)…
A: 4.45 Given molecules and ions, (a) ClF(b)…
Q: SE 2. Balance the following reactions using oxidation number method. CHARACTER F2(8) + Al(s)→ F(ag)…
A:
Q: The oxidation number of chlorine in its compound can lie between : a 0 to 7 b -1 to 7 c -2…
A: Chlorine is an electronegative element of group 17 (halogen family). It has seven electrons in its…
Q: Oxidation number method. Balance the equation by the oxidation number method. Mn02 + HCL = MnCl2 +…
A:
Q: Balance the reactions below using the change in oxidation number method. Show complete solutions.…
A: Redox reactions are the combination of reduction and oxidation reactions. The type of reaction in…
Q: 1. Hydrogen sulfide is an unpleasant constituent of "sour" natural gas. When this gas is burned in…
A:
Q: Some chemical reactants are listed in the table below. Complete the table by filling in the…
A:
Q: Assign oxidation states to each atom in each element, ion, orcompound.a. Ag b. Ag+ c. CaF2d. H2S e.…
A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…
Q: The oxidation number of an element may differ depending on whether or not it is contained within a…
A: True Because the oxidation number of an atom in a neutral free element is zero.
Q: Assign oxidation states to the elements whose atoms are underlined in each of the following…
A: The electrons that are transferred during a reaction by the element to another compound, is called…
Q: balance the ff. by change in oxidation state method A. Zn + HNO3 -> Zn(NO3)2 + N2O + H2O
A: Here the oxidation state of Zn increases by +2 while the oxidation state of N decreases by -4. Thus…
Q: Some chemical reactants are listed in the table below. Complete the table by filling in the…
A: Oxidation state - The total number of electrons that an atom either gains or loses in order to form…
Q: Some chemical reactants are listed in the table below. Complete the table by filling in the…
A: Answer:- this question is answered by using the simple concept of calculation of oxidation state…
Q: Balance the following reactions by the oxidation number method -1, + HNO, - HIO, + NO, + H,0 - HBr +…
A: Here we have to balance the following ionic equation by oxidation number method .
Q: In which reaction does the oxidation number of hydrogen change? A CaO (s) + H2O (/) → Ca(OH)2 (s) B)…
A: We have to identify the following given reactions in which the reaction does the oxidation number of…
Q: Balance the following equations using Oxidation Number method and explain how they are the same in a…
A:
Q: Balance this equation using oxidation method H2SO4 + FeSO4 + HNO3 = Fe2(SO4)3 + H2O + NO2
A:
Q: Assign oxidation states to each atom in each element, ion, or compound CuCl2 HSO4^- Cr2O7^2-
A: Given :- CuCl2 HSO4- Cr2O72- To assign :- Oxidation state of each atom in the given compounds
Q: Na2S203 + 12 →Nal+Na2s406|
A: Given reaction is : Na2S2O3 + I2 ------> NaI + Na2S4O6 Balancing the reaction by using only…
Q: The oxidation numbers of C in H2C2O4 and CH4 are ____ and ____, respectively. A) +4,-4 B) +3,0…
A: Oxidation number or state is the number of electrons that are either gain or lose by an atom in a…
Q: Assign oxidation numbers to all the atoms or ions in each of the following reactions. Then identify…
A: we know that increase in positive charge or loss of electron is oxidation and decrease in positive…
Q: Show the change in oxidation number in the following (in other words, give the number of electrons…
A: The number of electrons gained or lost by the atom has to be given,
Q: Which of the following has the correct assignment of oxidation numbers? a. Fe₂O3 (Fe: 2+, O: 2-) b.…
A:
Q: In which reaction does the oxidation number of oxygen increase? A) Mgo (s) + H2O (I) → Mg(OH)2 (s) B…
A: In the decomposition of H2O the hydrogen gas and oxygen gas is evolved At initial the oxidation…
Q: Give the oxidation numbers of all the elements of the following compounds. Show complete solutions.…
A: Given:- Give the oxidation numbers of all the elements of the following compounds. Show complete…
Q: Pb + 2Fe+2Fe2+ + Pb2+ bove reaction, the oxidation state of lead changes from ( to any electrons are…
A: The given reaction is, Pb + 2Fe3+ →2Fe2+ + Pb2+
Q: a) Using Oxidation Number Method MnO4 + H* + Cl → Mn2+ + Cl2 + H20 b) Using Half-Reaction Method…
A: MnO4- + H+ + Cl- -----> Mn+2 + Cl2 +H2O Cr+3 + ClO3- -----> Cr2O72- + Cl-
Q: What are the oxidation states of each element in the following compounds: (write them above each…
A: Oxidation state of an element can be calculated by considering the bond to be perfectly ionic and…
Q: The oxidation number of S is S2O62- is __. a) +4 b) +5 c) +3 d) +6
A: In S2O62- two oxygen atom are bonded with one sulphur by double bond and one oxygen by single bond .…
Q: 3. Determine the oxidation number for the indicated element in each of the following substances: (a)…
A:
Q: assign oxidation states to the elements in the following compounds or ions: a. KNO3 b.AlH3…
A: We have to assign oxidation states to the elements in 4 compounds.
Q: In the unbalanced equation, C4H10(l) + Cr2O72-(aq) + H+(aq) H6C4O4(s) + Cr3+(aq) + H2O(l), the…
A: Given equation is C4H10(l) + Cr2O72-(aq) + H+(aq) = H6C4O4(s) + Cr3+(aq) + H2O(l)
Q: Give the oxidation number for each element in the following compounds: ce e ooLd ednapoue A. Rb2S…
A:
Q: Which of the following is a redox reaction? O a. 2KB + F2 2KF + Br2 O b. 2HCI+ Mg(OH)2→2HOH + MgCl2…
A:
Q: In the conversion of Br2 to BrO3 , the oxidation state of Br changes from a 0 to 5 b 0 to -3 c 1…
A: Oxidation number is the charge that an atom present in a compound feels when all the other ions are…
Q: The oxidation number of each atom in ammonium sulfite, (NH4)2SO3, is, respectively= -6, +4, +6, -6 O…
A: The most stable oxidation number of H and O atoms is +1 and -2 respectively. The given compound gets…
Q: Assign oxidation states to each atom in each of the following species D. HCl E. PO4 3- F. CrO4 2-
A: The total number of electrons required to form a chemical bond by either losing or gain of electrons…
Q: Write the oxidation number (same as oxidation state) for the designated atoms (in boldface and…
A: To find oxidation state.
Q: Assign oxidation states to the elements whose atoms are underlined in each of the following…
A: The oxidation state of a pure compound or pure element is always taken as 0. The oxidation state of…
Q: Determine the oxidation number for each element of the following substances. 1) SO3 2) COC2 3)…
A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.…
Q: Balance using oxidation number method, KCl and CrCl3 are aqueous K₂Cr₂O₇ + HCl ---> KCl +…
A: We have to balance given redox reaction using oxidation number method
Q: The oxidation number of nitrogen given for all the following species is correct except a. N2 (0). b.…
A: The oxidation number is the residual charge left on an atom in a compound when all other species are…
Q: Assign oxidation states to each atom in each of the following species A. He B. Al3+ C. Na2O
A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…
Q: Balance the following equations using Oxidation Number method and explain how they are the same in a…
A: A reaction, where the oxidation and reduction reactions are taking place simultaneously, is known as…
Q: Assign oxidation states to each atom in each element, ion, or compound.a. Cl2 b. Fe3+ c. CuCl2d. CH4…
A: Since your question is multiple sub-parts. So according to our norms, we will solve only the first…
Q: I2(s) + OCl-(aq) → IO3-(aq) + Cl-(aq) Referring to the equation above, what is the oxidation number…
A:
Q: alance the following redox reaction using the oxidation number method. CrO2 ^ - +ClO^ - +OH^ -…
A: Oxidation number method for balancing redox reaction Assign oxidation numbers to the reactants and…
Determine the oxidation number of each atom:
H2O:
CH4:
CO3 2- :
NH4+:
PO4 3- :
Cl2:
Fe:
Step by step
Solved in 3 steps with 2 images
- Nickel(II) sulfate solution reacts with sodium hydroxide solution to produce a precipitate of nickel(II) hydroxide and a solution of sodium sulfate. Write the molecular equation for this reaction. Then write the corresponding net ionic equation.Elemental bromine is the source of bromine compounds. The element is produced from certain brine solutions that occur naturally. These brines are essentially solutions of calcium bromide that, when treated with chlorine gas, yield bromine in a displacement reaction. What are the molecular equation and net ionic equation for the reaction? A solution containing 40.0 g of calcium bromide requires 14.2 g of chlorine to react completely with it, and 22.2 g of calcium chloride is produced in addition to whatever bromine is obtained. How many grams of calcium bromide are required to produce 10.0 pounds of bromine?Triiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution: IO3(aq) + I(aq) I3(aq) Triiodide ion concentration is determined by titration with a sodium thiosulfate (Na2S2O3) solution. The products are iodide ion and tetrathionate ion (S4O6). a. Balance the equation for the reaction of IO3 with I ions. b. A sample of 0.6013 g of potassium iodate was dissolved in water. Hydrochloric acid and solid potassium iodide were then added. What is the minimum mass of solid KI and the minimum volume of 3.00 M HQ required to convert all of the IO3 ions to I ions? c. Write and balance the equation for the reaction of S2O32 with I3 in acidic solution. d. A 25.00-mL sample of a 0.0100 M solution of KIO. is reacted with an excess of KI. It requires 32.04 mL of Na2S2O3 solution to titrate the I3 ions present. What is the molarity of the Na2S2O3 solution? e. How would you prepare 500.0 mL of the KIO3 solution in part d using solid KIO3?
- Chlorine gas was first prepared in 1774 by C. W. Scheele by oxidizing sodium chloride with manganese(IV) oxide. The reaction is NaCl(aq) + H2SO4(aq) + MnO2(s) Na2SO4(aq) + MnCl2(aq) + H2O(l) + Cl2 (g) Balance this equation.Write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in each reaction? mg src=Images/HTML_99425-7-17ALQ_image001.jpg alt="" align="top"/> mg src=Images/HTML_99425-7-17ALQ_image002.jpg alt="" align="top"/>Gold can be dissolved from gold-bearing rock by treating the rock with sodium cyanide in the presence of oxygen. 4 Au(s) + 8 NaCN(aq) + O2(g) + 2 H2O() 4 NaAu(CN)2(aq) + 4 NaOH(aq) (a) Name the oxidizing and reducing agents in this reaction. What has been oxidized, and what has been reduced? (b) If you have exactly one metric ton (1 metric ton = 1000 kg) of gold-bearing rock, what volume of 0.075 M NaCN, in liters, do you need to extract the gold if the rock is 0.019% gold?
- The mineral dolomite contains magnesium carbon-ate. This reacts with hydrochloric add. MgCO3(s) + 2 HCl(aq) CO2(g) + MgCl2(aq) + H2O() (a) Write the net ionic equation for this reaction and identify the spectator ions. (b) What type of reaction is this?The Behavior of Substances in Water Part 1: a Ammonia, NH3, is a weak electrolyte. It forms ions in solution by reacting with water molecules to form the ammonium ion and hydroxide ion. Write the balanced chemical reaction for this process, including state symbols. b From everyday experience you are probably aware that table sugar (sucrose), C12H22O11, is soluble in water. When sucrose dissolves in water, it doesnt form ions through any reaction with water. It just dissolves without forming ions, so it is a nonelectrolyte. Write the chemical equation for the dissolving of sucrose in water. c Both NH3 and C12H22O11 are soluble molecular compounds, yet they behave differently in aqueous solution. Briefly explain why one is a weak electrolyte and the other is a nonelectrolyte. d Hydrochloric acid, HCl, is a molecular compound that is a strong electrolyte. Write the chemical reaction of HCl with water. e Compare the ammonia reaction with that of hydrochloric acid. Why are both of these substances considered electrolytes? f Explain why HCl is a strong electrolyte and ammonia is a weak electrolyte. g Classify each of the following substances as either ionic or molecular. KCl NH3 CO2 MgBr2 HCl Ca(OH)2 PbS HC2H3O2 h For those compounds above that you classified as ionic, use the solubility rules to determine which are soluble. i The majority of ionic substances are solids at room temperature. Describe what you would observe if you placed a soluble ionic compound and an insoluble ionic compound in separate beakers of water. j Write the chemical equation(s), including state symbols, for what happens when each soluble ionic compound that you identified above is placed in water. Are these substances reacting with water when they are added to water? k How would you classify the soluble ionic compounds: strong electrolyte, weak electrolyte, or nonelectrolyte? Explain your answer. l Sodium chloride, NaCl, is a strong electrolyte, as is hydroiodic acid, HI. Write the chemical equations for what happens when these substances are added to water. m Are NaCl and HI strong electrolytes because they have similar behavior in aqueous solution? If not, describe, using words and equations, the different chemical process that takes place in each case. Part 2: You have two hypothetical molecular compounds, AX and AY. AX is a strong electrolyte and AY is a weak electrolyte. The compounds undergo the following chemical reactions when added to water. AX(aq)+H2O(l)AH2O+(aq)+X(aq)AY(aq)+H2O(l)AH2O+(aq)+Y(aq) a Explain how the relative amounts of AX(aq) and AY(aq) would compare if you had a beaker of water with AX and a beaker of water with AY. b How would the relative amounts of X(aq) and Y(aq) in the two beakers compare? Be sure to explain your answer.One way of determining blood alcohol levels is by performing a titration on a sample of blood. In this process, the alcohol from the blood is oxidized by dichromate ions (Cr2O72-) according to the following net ionic equation: C2H5OH+2Cr2O72+16H+2CO2+4Cr3++11H2O A 10.00-g sample of blood was drawn from a patient, and 13.77 mL of 0.02538 M K2Cr2O7 was required to titrate the alcohol. What was the patient’s blood alcohol level? (See the previous problem for definition of blood alcohol level. K2Cr2O7 is a strong electrolyte, so it dissociates completely in solution.)