help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working! Solid aluminum (Al) and chlorine (Cl2) gas react to form solid aluminum chloride (AICI). Suppose you have 13.0 mol of Al and 11.0 mol of Cl, in a reactor.Calculate the largest amount of AICI, that could be produced. Round your answer to the nearest 0.1 mol.AmoOx10GDW

Given:Moles of Al = 13.0 mol (3 significant figures)Moles of Cl2 =…

Solid aluminum (Al) and chlorine (Cl2) gas react to form solid aluminum chloride (AICI). Suppose you have 13.0 mol of Al and 11.0 mol of Cl, in a reactor. Calculate the largest amount of AICI, that could be produced. Round your answer to the nearest 0.1 mol. Amo Ox10 G D W

Solid aluminum (Al) and chlorine (Cl2) gas react to form solid aluminum chloride (AICI). Suppose you have 13.0 mol of Al and 11.0 mol of Cl, in a reactor. Calculate the largest amount of AICI, that could be produced. Round your answer to the nearest 0.1 mol. Amo Ox10 G D W

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 132AE: Many cereals are made with high moisture content so that the cereal can be formed into various...

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Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?
The space shuttle environmental control system handles excess CO2 (which the astronauts breathe out; it is 4.0% by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets to form lithium carbonate, Li2CO3, and water. If there are seven astronauts on board the shuttle, and each exhales 20. L of air pee minute, how long could clean air be generated if there were 25,000 g of LiOH pellets available for each shuttle mission? Assume the density of air is 0.0010 g/mL.
3.50 A test of an automobile engine's exhaust revealed that g of NO2 was emitted in 10 minutes of operation. How many moles of NO2 would this engine release if it were used for a 45-minute commute, assuming that this mea- sured number is representative of the emission under all circumstances?
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
One way to remove nitrogen oxide (NO) from smoke-stack emissions is to react it with ammonia. 4NH3(g)+6NO(g)5N2(g)+6H2O(l) Calculate (a) the mass of water produced from 0.839 mol of ammonia. (b) the mass of NO required to react with 3.402 mol of ammonia. (c) the mass of ammonia required to produce 12.0 g of nitrogen gas. (d) the mass of ammonia required to react with 115 g of NO.
4.80 The reaction shown below is used to destroy Freon-12 (CF2Cl2), preventing its release into the atmosphere. What mass of NaF will be formed if 250.0 kg of CF2Cl2 and 400.0 kg of Na2C2O4 are heated and allowed to react to completion? CF2Cl2+2Na2C2O42NaF+2NaCl+C+4CO2
Consider the chemical reaction 2 S + 3 O2 → 2 SO3. If the reaction is run by adding S indefinitely to a fixed amount of O2, which of these graphs best represents the formation of SO3? Explain your choice.
4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
4.21 Ammonium nitrate, NH4NO3, will decompose explosively to form N2, O2, and H2O, a fact that has been exploited in terrorist bombings. What mass of nitrogen is formed by the decomposition of 2.6 kg of ammonium nitrate?
ou know that chemical A reacts with chemical B. You react 10.0 g A with 10.0 g B. What information do you need to know to determine the amount of product that will be produced? Explain.
4.72 The picture shown depicts the species present at the start of a combustion reaction between methane, CH4 and oxygen, O2 (a) What is the limiting reactant? (b) Draw the resulting state after this set of reactants has reacted as far as possible.
2. If only 13.6 g of methane is obtained, what is the percent yield of this gas? 34.1% 97.8% 325% 8.83%

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