! ( give step by step explanation) 8. Make a 4-8-10 fertilizer using the following chemicals as starting materials:NaNO3, a phosphate compound containing 15% available P2O5, KCI, and an inertfillerHow many kilograms of each of these materials will be required to make 1000kg offertilizer?(answer: 243kg NaNO3; 533kg phosphate compound; 158kg KCI; 66kg of filler)

Answered: Image /qna-images/answer/c0bdef37-2292-4e58-833a-bbc0fa6837c0.jpg

Answered: Make a 4-8-10 fertilizer using the…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 3CR

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Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
4.19 How many metric tons of carbon are required to react with 7.83 metric tons of Fe2O3 according to the following reaction? 2Fe2O3+3C3CO2+4Fe How many metric tons of iron are produced?
4.61 What is actually measured by the octane ratings of different grades of gasoline?
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.
A. Given the formulas of the reactants, supply the missing products, identify the type of reaction, and balance the equation. (1 pt each) 1. Reaction NazC204 + H2SO4 →. : Type of reaction : Balanced equation (2 pts) : 2. Reaction FeCl3 + KAFE(CN)6 → + KCI : Type of reaction : Balanced equation (2 pts) : 3. Reaction NHẠCI - + HCI : Type of reaction Balanced equation (2 pts) : 4. Reaction Na + Cl2 → Type of reaction Balanced equation (2 pts) : 5. Reaction Ni + AGNO3 → : Type of reaction : Balanced equation (2 pts) :
What quantity of carbon dioxide, CO2 (in grams) would be required to convert 5.60 g of 2-bromopropane to the carboxylic acid named isobutyric acid? [Enter a value with 3 sig figs and do not include any units] 1. Mg, Et,O 2. CO2 3. Н" он Br 2-bromopropane (MW = 122.9 g/mol) isobutyric acid (MW = 88.05 g/mol)
For every one molecule of NaHCO3(s) there is one molecule of CO2(g) that forms: NaHCO3(s) + CH3CO2H(aq) --> CO2(g) + H2O(l) + NaCH3CO2(aq) This means that if we know how many moles of gas we need, we need the same number of moles of sodium bicarbonate to produce it. Now, we need something to fill with gas. I'll be filling a 1-quart sealable plastic bag. 1 quart is 946 mL (0.946 L). We can use the ideal gas law to determine how much gas (in moles) is needed to fill 946 mL. Remember there are four variables for the ideal gas law. Ideal Gas Law: PV = nRT P = pressure: typically 715 mm Hg in Spokane <-- unit dictates which R to use V = volume: 1 quart bag = 0.946 L <-- must be in Liters T = room temperature: 20 °C in my lab, +273 = 293 K <-- must be Kelvin n = moles: what we are solving for I used atmospheric pressure in mm Hg, so I'll have to pick the R value with "mm Hg" in the units: R = 62.4 L × m m H g K × m o l Now, use these values to calculate how many moles of…
Chlorination of methane is shown as: Ch4 + Cl2 = CH3Cl + HClIf the feed contains 40% CH4, 50% Cl2 and 10%N2 and 67% of the limiting reactant is converted... Composition of methyl chloride(in moles) in the product? CHOICES: 26.8 49.2 55.4 67.9 Composition of nitrogen(in moles) in the product? CHOICES: 9 10 11 12
* What amount (in mol) and what mass (in kg) of carbon dioxide are produced when 20 gallons (approximately 2.0 x 10' kg) of octane (C3H18) is combusted? C3H18(1) +O2(g) CO2(g) + H;O(1) A: 1.4 x 10°; 62
Consider the following reaction: 6HCI + 2AI→ 2AICI3 + 3H2 Calculate the mass (in grams) of AICI3 produced by reacting 19 g of HCI and 15 g of Al. (MW (g/mol): HCl = 36.5, Al = 27, AICI3 = 133.3, H2 = 2) Express your answer with 1 decimal place. A
710 10. The formula of rust may be represented most simply as Fe(OH)3. The balanced equation when iron corrodes is: Try @home d. 60 e. 150 Page | 4 4Fe +302 + 6H₂O → 4Fe(OH)3 a. (2 points) What are the percentages by weight of the elements in rust? b. 5-points) How many grams of rust are formed when one kg of iron corrodes?

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