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- O Select the strongest acid. O I— ④SH HOH H OH IChlorophyll has the chemical formula C55H72MgN4O5 convert 1.3 kilograms of chlorophyll to moleculesConsider the reaction. heat 2 Al(s) + Fe,03(s) Al,0;(s) + 2 Fe(l) If 11.5 kg Al reacts with an excess of Fe,O3, how many kilograms of Al,O, will be produced? mass of Al,0, produced:
- Soda ash (sodium carbonate) is widely used in the manufacture of glass. Prior to the environmental movement much of it was produced by the following reaction. CaCO3 + 2 NaCl → Na2CO3 + CaCl2 Unfortunately, the byproduct calcium chloride is of little use and was dumped into rivers, creating a pollution problem. As a result of the environmental movement, all of these plants closed. Assume that 125g of calcium carbonate (100.09 g/mol) and 125 g of sodium chloride (58.44 g/mol) are allowed to react. Determine how many grams of useful sodium carbonate (105.99 g/mol) will be produced. How many grams of useless calcium chloride (110.98 g/mol) will be produced? You should also determine how many grams of excess reactants are left (indicate which one is the limiting reactant)Hydrogen is manufactured on an industrial scale by this sequence of reactions: CH4 (g) + H₂O(g) = CO (g) + 3H₂(g) CO(g) + H₂O(g) = CO₂ (g) + H₂(g) The net reaction is: CH4 (g) + 2 H₂O(g) = CO₂(g) + 4H₂(g) Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K₁ and K₂. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K = 0 ロ・ロ X K₁ K₂ 4 KKXI What is the reaction of the following reaction? 1. Hg(OAc)₂, H₂O x 2. NaBH4, NaOH OH OH x OH
- For the following chemical reaction, N2 (g) + 3 H2 (g) → 2 NH3 (g) If 15 molecules of nitrogen gas and 12 molecules of hydrogen gas react together what will be left in the container at the end of the reaction.esc O Gases Solving for a gaseous reactant The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 8 FI 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 49.0 mL of dioxygen gas are produced by this reaction, at a temperature of 120.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Round your answer to 3 significant digits. Explanation @ S 38² Check F2 https://azinsight.adsrvr.org/track/clk?imp=fbec12b0-7f3d-4127-929d-a59782e61fbb&ag=r735012&sfe=1788cd47&sig=PCK7icABpePPZol9wV_E9gKn0P16FOTr7R3rMUmfWw.&crid=2zvfx50b&cf=5773664&fq=0&t=2&td_s=www.c #3 80 F3 $ 4 a F4 do LO %…Narceine is a narcotic in opium that crystallizes from solution as a hydrate that contains 10.8 mass % water and has a molar mass of 499.52 g/mol. Determine x in narceine⋅xH2O.
- How many grams of NBr3 can be made from 2.22 x 10-2 moles of Br2 ? N2 + 3 Br2 → 2 NB13 + 44.0 kJ The molar mass of NBR3 is mol NBr3 (2.22 x 102 mol Br2)(- mol NBR3 %3D mol Br2 g NBr3 mol NBr3 (- g NB13 mol NBr3 а. 1 b. 2 С. 3 d. 4 е. 5 f. 253.719 g. 3.76 x 10° h. 3.26 x 103 i. 44.0 j. 1.48 x 10-2 k. 9.77 x 103 1. 4.44 x 102 m. 6.66 х 102 n. 500.0 o. 556 р. 90.0 q. 3.2852 r. 159.81 S. 28.013 t. 1.750 u. 0.8750 v. 13.0 w. 0.46306 х. 1.3892 у. 24.5 z. 38.5 аа. 2.190 bb. evolved cc. absorbed dd. exothermic ee. endothermicA OH E CN B F NH₂ } с XOXX H hy D en HConsider the reaction. heat 2 Al(s) + Fe,0,(s) Al,03(s) + 2 Fe(1) If 11.5 kg Al reacts with an excess of Fe,O2, how many kilograms of Al,0, will be produced? mass of Al,0, produced: kg
