Consider the formation of gibbsite from dissolved aluminum as depicted below: Al3+    +       OH- -->         Al(OH)3 (gibbsite) a) balance this reaction (if necessary) b) predict how many mg of Al(OH)3 would be formed if 3 mg of Al3+ are dissolved in 1 l of water and “unlimited” OH- is available (assume this reaction goes completely to the right; there’s no worry about equilibrium dissolved Al3+).

In iron smelting, what are the possible chemical equations that will involve CaO if CaO is part of the iron ore?

In theory, sodium (Na) metal could be used in place of magnesium (Mg) in the preparation of titanium metal from TiO2. From Lecture 3-1, slide 4:  TiO2  +  2 Mg  -->  2 MgO  +  Ti Which of the following statements would be true if sodium was used instead of magnesium? Group of answer choices None of the other three statements are true. The reaction would not proceed with sodium because sodium oxide (analogous to the MgO product that forms) can't exist You would need 4 moles of Na because the sodium oxide product has a formula of Na2O. The reaction could not be done because sodium metal does not actually exist

The answer in the box is incorrect. Please find the correct answer. Thank you!

Predict the products and balance the equation: No Spacing between coefficients and elements/compounds. Place a "1" where assumed. Hint: Single Replacement Oxidation Numbers: H+1 Fe +4 O-2 H2+ Fe304 ---> +.

I only need help with question C

plz explain step by step in detail

Consider a modification to the Hall-Heroult process for aluminum production, where we keep things the same but replace the carbon electrode by something inert. The original process requires three electrons to produce one atom of Al metal and is: (1/2) Al½O3 + (3/4) C → Al + (3/4) CO2 Suppose that the new process also requires three electrons and is (1/2) Al,O; → Al + (3/4) O2 If the energy, E, produced from the reaction C + O2 → CO2 is 4.08 eV per carbon atom, how much would the voltage need to be increased in order produce aluminum assuming that the energy from the oxidation of carbon to carbon dioxide is replaced by electrical energy in the process?

Pp

[20.100] Gold exists in two common positive oxidation states, +1 and +3. The standard reduction potentials for these oxida- tion states are Au*(aq) + e Au(s) Eed = +1.69 V > Au*(ag) + 3 e → Au(s) Ered = +1.50 V (a) Can you use these data to explain why gold does not tar- nish in the air? (b) Suggest several substances that should be strong enough oxidizing agents to oxidize gold metal. (c) Miners obtain gold by soaking gold-containing ores in an aqueous solution of sodium cyanide. A very soluble com- plex ion of gold forms in the aqueous solution because of the redox reaction 4 Au(s) + 8 NaCN(aq) + 2 H,O(1) + O2(g) 4 Na[Au(CN),](aq) + 4 NaOH(aq) > What is being oxidized and what is being reduced in this reac- tion? (d) Gold miners then react the basic aqueous product solution from part (c) with Zn dust to get gold metal. Write a balanced redox reaction for this process. What is being oxi- dized, and what is being reduced?