A mass of 500 grams + (Your Registration number) of Butane (C4H10) is completely Oxidized into Carbon Dioxide (CO2) and Water (H2O). The unbalance reaction is given as C4H10 + O2 → CO2 + H2O (i) Apply the knowledge of chemistry to balance the equation and (ii) Compute Mass of Carbon dioxide to be produced from 500 grams of Butane.

A mass of 500 grams + (Your Registration number) of Butane (C4H10) is completely Oxidized into Carbon Dioxide (CO2) and Water (H2O). The unbalance reaction is given as C4H10 + O2 → CO2 + H2O (i) Apply the knowledge of chemistry to balance the equation and (ii) Compute Mass of Carbon dioxide to be produced from 500 grams of Butane.

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter6: Thermochemisty

Section: Chapter Questions

Problem 6.159QP: The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by...

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he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per year. Acrylonitrile, the building block tor acrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: :math>2C3H6(g)+2NH3(g)+3O22C3H3N(g)+6H2O(g) l type='a'> Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: l> Mass Reactant msp;5.23102g propylene td> msp;5.00102g ammonia td> msp;1.00103g oxygen td> i>What mass of water is formed from your mixture? Calculate the mass (in grams) of each reactant after the reaction is complete.
You are supplied with 1150 kg ethanol (C2H5OH), together with methanol (CH3OH), potassium hydroxide (KOH) and ammonia (NH3). You are requested by a customer to produce methyl acetate (CH3COOCH3), potassium acetate (CH3COOK) and ammonium acetate (CH3COONH4) in mass forms. (a) Calculate the mole & mass of acetic acid (CH3COOH) converted from ethanol through excessive oxidation.
The Bayer process is the formation of aluminum hydroxide from metallic aluminum and sodium hydroxide heated to high temperatures. Al(s)+ 3NaOH(aq) -->Al(OH)3(s) + 3Na A manufacturing chemist observes that two distinctly different solids are present in the solutions after the reaction has come to completion. The chemist collected the following data: data table From the above information, identify the limiting and excess reagent, the supporting evidence, and suggest a method to increase the amount of product produced.
After balancing the chemical equation for the combustion in air of liquid C3H8O using the smallest possible whole number coefficients, what is the sum of the coefficients in the product side?
Please find the CO2 amount and show the calculation: Air composition (apprx) = 80% N2 and 20% O2 (mol basis only)Average molecular weight of Air = (0.8 x 28 + 0.2 x 32) = 29 g/mol (apprx) Math Sample:2kg pure charcoal (12C) is to be burnt completely with air. Find the air, CO2 andN2 amount in kg’s.Solution:C + O2 = CO2 (you must use a balanced equation)Therefore from the mole ratio of the reaction we write,C : O2 : CO2 = 1:1:1and from air composition we gotO2 : N2 : Air = 1:4:5 Given, 2 kg C = 2000 g/ (12 g/mol) = 166.67 mole CTherefore, similar mole of O2 required. So equivalent Air supposed to be 5times than the mole amount of O2 and released N2 will be 4 times than therequired O2. Therefore, Air amount = 5 x 166.67 moles= 833.34 moles= (833.33x29/1000) kg= 24.17 kg air Similarly N2 released amount will be = (166.67 x 4 x 28/1000) kg = 18.67 kgFind CO2 amount by yourself! (Isn’t it 7.34 kg?)
.5 Balance the reaction: ___ C6H14 (l) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (g) Then give the coefficient of oxygen gas.
Citric acid, C6H8O7, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is C12H22O11 + H2O + 3O2 --> 2C6H8O7 + 4H2O Using a metric ton(1000kg) of sucrose the expected yield is 1122Kg. On average if only 1036kg is produced, what is the % yield for this reaction?
A chemist carries out the reaction below and obtains 3.45g of iron Fe (Fe, MW=55.845g/mol). Fill in the blanks below to determine the percent yield of the reaction when 8.30g of Fe2O3 (MW= 159.69g/mol) and 3.50g of CO (MW=28.01G/mol)were used in the reaction. Fe2O3(s) + 3CO(g) = 2Fe(s) + 3CO2(g) Note that for two of the blanks, will be the same answer. 1. What would be the mass in grams of Fe produced based on the mass of Fe2O3 used? answer: (blank) 2. What would be the mass in grams of Fe produced based on the mass of CO used? answer: (blank) 3. What is the theoretical yield of Fe in grams? answer: (blank) 4. What is the limiting reagent? Enter the formula of compound. answer: (blank) 5. What is the percent yield of this reaction? answer: (blank)
The reaction mixture intially contains 4.0 g of ferrous ammonium sulfate hexahydrate, Fe(NH4)2(SO4)2 * 6H2O, and 50mL 1M oxalic acid. Determine the limiting reactant,Theoretical yield of the ferrous oxalate dihydrate, and The per cent yield of the ferrous oxalate dihydrate product.
22. A recipe for 1 cup of hollandaise sauce calls for ½ cup of butter, ¼ cup of hot water, 4 egg yolks, and the juice of a medium-sized lemon. How many cups of this sauce can be made from a pound (2 cups) of butter, a dozen eggs, 4 medium lemons, and an unlimited supply of hot water? Write an equation for making sauce, then use dimensional analysis and the process used in class for dealing with limiting reagents. How much of each ingredient are in excess?
4.4g KMnO4 is mixed with water and 1.3 of iodine powder is added to the mixture 0.14g of potassium iodide and a few little grams of potassium hydroxide what are the chemical equations of this reaction and the limiting reagent
GivenRaw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g precipitated sulfurWhereas the balanced chemical reaction, as given in the problem is: CaS5+2HCl => 4S + CaCl2 + H2Sa. Find the Mass to Mass Stoichiometry Calculation b. Upon solving A, find the LIMITING REAGENT, EXCESS REAGENT and the AMOUNT IN EXCESSc. Find the Percentage Yield from Problem Ad. Find the number of dosage form and packaging that can be produced from the stoichiometric calculation based on Problem A

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