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Write the K formula for the following reactions.
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- Hematite, Fe₂O3, is an important ore of iron. (An ore is a natural substance from which the metal can be profitably obtained.) The free metal is obtained by reacting hematite with carbon monoxide, CO, in a blast furnace. Carbon monoxide is formed in the furnace by partial combustion of carbon. The reaction is Fe₂O3(s) + 3CO(g) → 2Fe(s) + 3CO₂(g) How many grams of iron can be produced from 1.34 kg Fe₂03? g FeBalance the equation: Y2O3(s) + SO3(l) → Y2(SO4)3(s)Balance the chemical equation. CH() +150₂(g) → 12CO₂(g) + 6H₂O(g)
- HNO3(aq) + Fe(OH)3(s) →Balance the following chemical equation (if necessary): C6H6(1) + O2(g) → H2O(g) + CO2(g)One of the first steps in a method to process “yellowcake” uranium ore for nuclear fuel is to dissolve the material in nitric acid.: U3O8(s) + 8HNO3(aq) + 14H2O(l) → 3[UO2(NO3)2·6H2O](aq) + 2NO2(g) Each steel drum of yellowcake contains about 4.0 x 102 kg of ore. The mass percentage of U3O8 in the ore is 80.%. A truck can haul 43 drums of ore to the uranium refinery. How many moles of nitrogen dioxide “off-gas” (a pollutant that must be recovered) are produced per truckload of ore? Report your answer in scientific notation (format, 1.2E3 with a capital E to keep Blackboard happy) using 2 significant figures. Do not include units.
- Balance the following chemical equation (if necessary): SiO₂ (s) + C(s) → Si(s) + CO(g)Balance the equation: Ni(s) + H2O(l) + O2(g) → Ni(OH)2(s)What mass of methane is required to produce 1.130 kg of carbon dioxide during combustion? (Assume the reaction undergoes complete combustion.) CH4(g) + O2(g) → CO2(g) + H2O(g) O 411.8 g O 113.2 g O 24.5 g
- What mass, in grams, of C2H2 is needed to form 212.9 kg of CO2? Assume excess oxygen. 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)b The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the following steps: 4NH3(g) + 502(g) → 4NO(g) + 6H,O(g) (1) 2NO(g) + O2(g) → 2NO2(g) (2) 3NO2(g) + H20(1) → 2HNO3(aq) + NO(g) (3) Is the overall reaction exothermic or endothermic? exothermic endothermic22. Copper is obtained from sulfide ores through a two-step process consisting of roasting the ore in the presence of oxygen and heating the resultant copper(I) oxide with powdered carbon. The overall reaction is as follows: 2Cu2S (s) + 302 (g) + 2C (s) → 2SO2 (g) + 4Cu (s) + 2CO (g) Calculate the maximum yield of copper obtained from 1.60 kg of Cu2S. (Relative atomic mass: S, 32; O, 16; C, 12; Cu, 64) A. 0.26 kg В. 0.64 kg С. 0.96 kg D. 1.28 kg