Writing the net equation The extraction of aluminum metal from the aluminum hydroxide in bauxite ore by the Hall-Héroult process is one of the most remarkable success stories of late 19th century practical chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina and water: 2 Al(OH)3(s)-Al₂O3(s) + 3H₂O(g) In the second step, alumina and carbon react to form aluminum and carbon dioxide: 2 ALO,(s)+3 C(s)-4 Al(s) + 3 CO₂(g) Write the net 'chemical equation for the production of aluminum from aluminum hydroxide and carbon. Be sure your equation is balanced. The Co Op alo

The Haber Process, developed by Fritz Haber in 1909, was a revolutionary method for producing ammonia from elemental hydrogen and nitrogen on an industrial scale. Write a balanced equation showing the conversion from elemental nitrogen (N2) and hydrogen (H2) to ammonia (NH3). (Omit states-of-matter from your answer.)

Cryolite (Na3AlF6) is used in the commercial production of aluminum from ore. Cryolite itself is produced by the following reaction: 6 NaOH + Al₂O3 + 12 HF → 2 Na3AlF6 + 9 H₂O A mixture containing 420.0 kg of NaOH, 228.4 kg of Al2O3, and 600.0 kg of HF is heated to 950 °C until it reacts to completion. What is the maximum mass of Na3AlF6 formed? kg Na3AlF6

The titanium chloride then reacts with liquid magnesium at 900°C to givetitanium and magnesium chloride (MgCl2). Write a balanced chemicalequation for this step in the refining of titanium.

Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients.

Aluminum is produced commercially by the electrolysis of Al2 O3 in the presence of a molten salt. If a plant has a continuous capacity of 1.49 million A, what mass of aluminum can be produced in 3.00 h? Mass = g

Q2

Balance the following chemical equations (include the states of matter)     The hydrolysis of P4O10(s) with H2O(l) to produce phosphoric acid, H3PO4(l )

21. Nitric acid is manufactured in the Oswald process, which involves the catalytic oxidation of ammonia according to the following equations: (i) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) (ii) 2 NO(g) + O2(8) 2 NO2(g); (iii) 3 NO2(g) + H2O(1) → 2 HNO3(aq) + NO(g); (NO is fed back into the second reactor) (a) The above equations may be combined to yield the following equation. Balance this equation. NH3(g) +_O2(g) + _H2O(1) _HNO3(1) + _H,O(1) + NO(g) (b) What is the mole fraction of NH3 that becomes nitric acid in one reaction cycle? (c) How many kilograms of HNO3 will be produced in one reaction cycle from 1.00 m³ of NH3, measured at STP, if the overall yield is 92.0%? (d) If concentrated nitric acid contains 70.0% (by mass) of HNO3 and the solution has density of 1.48 g/mL, how many litters of concentrated nitric acid is produced in this process at the above reaction yield? (Answers: (b) 2/3; (c) 1.73 kg of HNO3; (d) 1.67 L)