4. Limestone containing 87% CaCO3, 6% MgCO3, 3% hematite, 2% silica andremaining water is calcined in hot water to vaporize the water and separate CO2 fromthe carbonates. The CaO and MgO created by the reaction leave in the solid calcine,along with hematite and silica. How many kilograms of calcine will be produced perton of limestone?

To calculate the amount of calcine produced per ton of limestone, we first need to determine the…

Answered: 4. Limestone containing 87% CaCO3, 6%…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter21: Chemistry Of The Nonmetals

Section: Chapter Questions

Problem 37QAP: Iodine can be prepared by allowing an aqueous solution of hydrogen iodide to react with manganese...

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Similar questions

Iodine can be prepared by allowing an aqueous solution of hydrogen iodide to react with manganese dioxide, MnO2. The reaction is 2I(aq)+4H+(aq)+MnO2(s)Mn2+(aq)+2H2O+I2(s) If an excess of hydrogen iodide is added to 0.200 g of MnO2, how many grams of iodine are obtained, assuming 100% yield?
A chemist dissolves a 1.497-g sample of a type of metal (an alloy of Sn, Pb, Sb, and Cu) in nitric acid, and metastannic acid, H2SnO3, is precipitated. She heats the precipitate to drive off the water, which leaves 0.4909 g of tin(IV) oxide. What was the percentage of [in in the original sample?
What volume of 0.250 M H2SO4 solution is required to neutralize a solution that contains 5.00 g of CaCO3?
The amount of sodium hypochlorite in a bleach solution can be determined by using a given volume of bleach to oxidize excess iodide ion to iodine; ClO- is reduced to Cl-. The amount of iodine produced by the redox reaction is determined by titration with sodium thiosulfate, Na2S2O3; I2 is reduced to I-. The sodium thiosulfate is oxidized to sodium tetrathionate, Na2S4O6. In this analysis, potassium iodide was added in excess to 5.00 mL of bleach (d=1.00g/cm3) . If 25.00 mL of 0.0700 M Na2S2O3 was required to reduce all the iodine produced by the bleach back to iodide, what is the mass percent of NaClO in the bleach?
Calcium oxide can be used to "scrub" carbon dioxide from air. What mass of CO2 could be absorbed by 1.25 g of CAO
Solid barium oxide and carbon dioxide gas are produced by the decomposition of solid barium carbonate BaCO3. Write a balanced chemical equation for this reaction.
is formed from... Br NH2 N-H (A) (B) (C) (D) (E) O Compounds B and E Compounds A and E Compounds C and D Compounds A and D
Solid boron can be extracted from solid boron oxide by reac- tion with magnesium metal at a high temperature. A second prod- uct is solid magnesium oxide. (a) Write a balanced equation for the reaction. (b) What mass of boron can be produced when 125 kg of boron oxide is heated with 125 kg of magnesium?
NaF and CaO.Which has the higher melting point and why?
4. Write balanced formation equations for the following, indicate proper states:| → N203(g) → C2H3F(g)
Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime (calcium oxide), which they produced by roasting limestone (calcium carbonate). 1. Write a balanced chemical equation, including physical state symbols, for the O-0 decomposition of solid calcium carbonate (CaCO2) into solid calcium oxide and gaseous carbon dioxide. da 2. Suppose 50.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 400.0 °C and pressure of exactly 1 atm, Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits. 0g Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy Accessibility MacBook Air DI 888 F9 F10 F7 F8 F3 F4 F5 F6 F1 23 2$ & の %24

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