[Review Topics] [References] Iron metal is obtained by reduction of iron(III) oxide with powdered aluminum. The reaction is highly exothermic, and the products are molten Al O3 (1) and Fe(l). Write the balanced equation for this reduction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)

[Review Topics] [References] Iron metal is obtained by reduction of iron(III) oxide with powdered aluminum. The reaction is highly exothermic, and the products are molten Al O3 (1) and Fe(l). Write the balanced equation for this reduction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Use standard reduction potentials to calculate the standard free energy change (ΔGº) for the reaction below at 25º. Report your answer in kilojoules.3 Ag2O (s) + 2 Cr(OH)3 (s) + 4 OH – (aq) ⟶ 6 Ag (s) + 2 CrO4 –2 (aq) + 5 H2O (l)ΔGº = Answer kJ
Identify the oxidizing and reducing agents in the skeletal (unbalanced) reaction. Then, balance the reaction, including the phase (solid, liquid, etc.) of each species. The reaction takes place in basic aqueous solution. Cl,0,(g) + H,0, (aq) Cio, (aq) + 0,(g) oxidizing agent reducing agent balanced equation:
Chlorine dioxide (ClO2), which is produced by the reaction below, has been tested as a disinfectant for municipal water treatment. 2 NaClO2(aq) + Cl2(g) → 2 ClO2(g) + 2 NaCl(aq) (a) Using data from the Standard Reduction Potentials table, calculate ℰ°, ΔG°, and K at 25°C for the production of ClO2. ℰ° V ΔG° kJ K (b) One of the concerns in using ClO2 as a disinfectant is that the carcinogenic chlorate ion (ClO3− ) might be a by-product. It can be formed from the following reaction. ClO2(g) → ClO3−(aq) + Cl−(aq) Balance the equation for the decomposition of ClO2. (Use the lowest possible coefficients. Include states-of-matter at 25°C and 1 atm in your answer.)
Consider the following reaction: Au + O2 +F2 → [0₂]*[AuF6] Assign oxidation numbers (ON) for each of the elements participating in the following reactions. Answer format: [ON(Au)], [ON(O₂)]. [ON(F2)]. [ON(O2)]. [ON(Au), ON(F)] O [0]. [-1], [0]. [+1]. [+5. -1] O [0]. [0], [0]. [+1]. [+1, -1] O [0], [0], [0]. [+1]. [+5, -5] O [0]. [0]. [0]. [+1]. [+5, -1]
i. Calculate the number of kilowatt-hours of electricity required to produce 1.0 x 103 kg of aluminum by electrolysis of Al* if the applied voltage is 4.50 V and the process is 45% efficient. (1 kWh = 3.6 x10® J and 1 J = 1C x 1V) ii. Disproportionation reaction is an oxidation-reduction reaction in which the same substance is oxidized and reduced. Complete and balance the following disproportionation reaction. Cl, (aq) Cr (aq) + CIO (aq) (basic solution)
Please balance equation
Balance the equation in basic conditions. Phases are optional. equation: SO3 + Co(OH)₂ → Co + SO 4
The thermite reaction is written below. Show that the heat released in this reaction is sufficient for the iron to be produced as molten metal. Find the enthalpy of formation of the overall reaction. Al(s) + Where: Al ΔΗ°F= 0 Al2O3 AHF -2076 Fe AHF 0 Fe2O3 AHF -745 Fe₂O3(s)- → Al₂O3(s) + Fe(1)
SbO3-(aq) is reduced to Sb3+(aq) by Ga(s) which is oxidised to Ga2O3(s). Complete a balanced equation that describes this.
calculate the amount of energy required to make 235 g of aluminum at a smelting temperature of 658°C
Solder is an alloy containing the metals tin and lead. A particular sample of this alloy weighing 1.50 g was dissolved in acid. All of the tin was then converted to the +2 oxidation state. Next, it was found that 0.368 g of Na2Cr2O7 was required to oxidize the Sn2+ to Sn4+ in an acidic solution. In the reaction, the chromium was reduced to Cr3+ ion.1. Write a balanced net ionic equation for the reaction between Sn2+ and Cr2O72- in an acidic solution.2. Calculate the number of grams of tin that were in the sample of solder.3. What was the percentage by mass of tin in the solder? Can you answer these questions for me and sort of explain how you got the answer. Redox reactions are giving me the blues.
Answer the four questions below related to the spontaneous redox reaction that occurs whenCr(OH)3(s) reacts with NO3–(aq) to produce CrO42–(aq)and NO2–(aq) under basic conditions. Write the balanced net ionic equation, including states of matter, for the overall reaction.