Which of the following metals would remain stable when placed in a dilute acid solution: zinc, magnesium, copper, or tin? Justify your answer.

For a particular redox reaction, BrO− is oxidized to BrO−3 and Fe3+ is reduced to Fe2+ . Complete and balance the equation for this reaction in basic solution. Phases are optional. balanced redox reaction:

CN–(aq) reacts with reacts with MnO4–(aq) to produce CNO–(aq) and MnO2(s).(i) What type(s) of reaction is this?(ii) Write a balanced chemical equation for this reaction.(iii) Which substance is the oxidizing agent?

Complete and balance the following reactions - assume they all go a. lead metal plus silver nitrate solutionb. chlorine gas plus sodium bromide solutionc. C7H16 plus oxygen gasd. Barium metal plus nitrogen gas

3. Copper (II) perchlorate undergoes a double displacement reaction with ammonium phosphate. Write the balanced equation

now you return to the test tube containing Group III ions. After testing, you have a pink precipitate. Explain the identity of the Group III ions and how you came to this conclusion

Substances A, B, and C can all act as oxidizing agents. In solution, A is green, B is yellow, and C is red. In the reactions in which they participate, they are reduced to A−, B−, and C− ions, all of which are colorless. You are given an unknown, colorless, solution that contains one of the following salts: NaA, NaB, NaC. In solution, each salt dissociates completely into the Na+ ion and the anion A−, B−, or C−. The Na+ ion is effectively inert. You are given the availability of solutions of A, B, and C, develop a simple procedure for identifying the salt that is present in your unknown.   Question 6 options:   React your unknown with NaA, NaB and NaC respectively. If a reaction occurs, your unknown is a better oxidizing agent than what you reacted it with. Use the oxidation strength order calculated in the previous question to determine your unknown.   React your unknown with NaA, NaB and NaC respectively. If a reaction occurs, your unknown is a worse…

6. The following reaction forms a white precipitate. Is this a redox reaction? AgNO3(aq) + HCl(aq) → HNO3(aq) + AgCl(s)

Write the balanced molecular chemical equation for the reaction in aqueous solution for copper(I) bromide and potassium sulfate. If no reaction occurs, simply write only NR.

An electrochemical change occurs when a strip of nickel is immersed in an acidified solution that contains dichromate ions. The colour change that occurs as the reaction above proceeds is: Select one: Green to colourless Orange to green Colourless to green Green to orange Which of the following metals could have been used instead of nickel in order to maintain the original colour of the solution described above? Select one: O Gold Magnesium O Copper Cadmium Which of the following entities will react spontaneously with Cd(s) but not with Ni(s)? Select one: Sn²+ (aq) Cr²+ (aq) Coz+(aq) H₂Se(aq)