Answered: Consider the reaction. heat 2 Al(s) +…

Consider the reaction. heat 2 Al(s) + Fe,O,(s) Al, 0,(s) + 2 Fe(1) If 23.1 kg Al reacts with an excess of Fe, O,, how many kilograms of Al,O, will be produced? kg mass of Al, O, produced:

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...

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Consider the reaction. 2Al(s)+Fe2O3(s)−→−heatAl2O3(s)+2Fe(l)2Al(s)+Fe2⁢O3⁡(s)→heatAl2⁢O3⁡(s)+2Fe(l) If 18.3 kg Al18.3 kg Al reacts with an excess of Fe2O3,Fe2⁢O3, how many kilograms of Al2O3Al2⁢O3 will be produced? mass of Al2O3Al2⁢O3 produced:
Balance the following chemical equation (ifnecessary):C6H6O(I) + O2(g) -> H20 (g) + CO2 (g)
The combustion of 1.66 g ultrafine aluminum in air results in 2.97g of a product, which is a mixture of 80 % aluminum oxide and 20% aluminum nitride (% by mass) Use the empirical formula of aluminum oxide and find the formula for aluminum nitride. Report the molar amount of aluminum oxide: ттol so that the molar amount of aluminum in the nitride can be found as: тmol and the molar amount of nitrogen is: ттоl so that the ratio of aluminum to nitrogen can be found to be: а.и.
1. For, 2 Al (s) +3 CuCl2 (aq) →2 AICI3 (aq) + 3 Cu (s) (a) Find the moles of Cu formed by using 5.4 g Al. Given amount Answer Work (by dimensional analysis) and units with units (b) Find the moles of Cu created in the reaction with 26.0 g of CuCl2. Given amount Answer Work (by dimensional analysis) and units with units (c) Which reactant is the limiting reactant? (Al or CuCl,)
Consider the reaction. heat 2 Al(s) + Fe,O3(s) Al,0;(s) + 2 Fe(1) If 11.5 kg Al reacts with an excess of Fe, O,, how many kilograms of Al, O, will be produced? mass of Al, 0, produced: 5.75 kg Incorrect
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) 2 NH3 (8) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH3 (g) + 20₂(g) - HNO3(g) + H₂O(g) Suppose the yield of the first step is 81.% and the yield of the second step is 88.%. Calculate the mass of hydrogen required to make 3.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. 0 x10 00 X
3. This illustration shows the energy change during the following reaction: CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) Potential energy (E₂) Energy Changes during an Exothermic Reaction in an Open System 1 mol CH₂(g) 2 mol O₂(g) (reactants) system AE 1 mol CO₂(g) 2 mol H₂O(g) (products) energy surroundings Which statement is true? A. The products contain more energy than the reactants. B. The reactants contain more energy than the products. C. The potential energy of the system is increasing. D. No energy changes are occurring.
The thermite reaction between powdered aluminum and iron(III) oxide, 2A1+ Fe2O3 → Al2O3 + 2Fe produces so much heat the iron that forms is molten. Suppose that in one batch of reactants 4.35 mol of Al was mixed with 2.15 mol of Fe2O3 (a) Which reactant, if either, was the limiting reactant? O Fe2O3 ○ Al O Fe O Al2O3 eTextbook and Media (b) Calculate the number of grams of iron that can be formed from this mixture of reactants. g Fe
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N2(g) +3H2(g) =2NH3(g) In the second step, ammonia and oxygen react to form, nitric acid (HNO3) and water: NH3(g) +2O2(g) = HNO3(g) +H2O(g). Suppose the yield of the first step is 65% in the yield of the second step is 78%. Calculate the mass of nitrogen required to make 9.0 kg of nitric acid. Be sure your answer has a unit symbol and is rounded to two significant digits.
Your lab partner accidentally mixed some sodium chloride with your sample of Epsom salts (MgSO₄･7H₂O). You want to make a standard solution of magnesium ion, and this is the only sample of a magnesium salt you have. To determine the amount of magnesium salt in the mixture, you heat 100.00 g to drive off the water of hydration and find that the anhydrous mixture has a mass of 55.25 g. What is the mass in grams of the original salt mixture that you must add to 1.000 L of water to make a 0.1000 M solution of Mg²⁺ ion?
The enthalpy for combustion for ethanol at 298 K is -1370.7 kJ/mole and occurs via the following balance chemical reaction. C2H6O (l) + 3 O2 (g) ⟶ 2 CO2 (g) + 3 H2O (g) If 0.461 grams of ethanol are combusted in the presence of 1.28 g of O2, answer the following. a. How many grams of CO2 could be produced? b. How much heat is released? c. What is the change in internal energy (ΔU)?
Up [References] Ethanol, the alcohol used in automobile fuels, is produced by the fermentation of sugars present in plants. Corn is often used as the sugar source. The following equation represents the fermentation of glucose, the sugar in corn, by yeast to produce ethanol and carbon dioxide. C6 H12 O6 (aq) → → 2C2H; OH(aq) + 2CO2 (g) Ethanol is combusted in an automobile engine according to the equation C2H; OH(1) + 302(g) → 2CO2 (g) + 3H2O(g) What would be the total volume of CO2 gas formed at STP when 4.45 kg of sugar is fermented and the ethanol is then combusted in an automobile engine? Volume = L Submit Answer Try Another Version 3 item attempts remaining