Pleasssssseeee solve this question in cheeemsirty, thankss sir What is the volume of CO2 gas produced at a pressure of 645 torr and atemperature of 800 K when 45.0 g of calcium carbonate (CaCO3, molar mass= 100.1 g/mol) decomposes completely according to the following reaction?CaCO →→CaO(s) + CO2(g)a) 34.8 Lb) 30.9 Lc) 27.1 Ld) 23.2 Le) 19.3 L

Answered: Image /qna-images/answer/f1ee6636-93aa-44f8-bdf0-dd9022086302.jpg

Answered: What is the volume of CO2 gas produced…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 46QRT

See similar textbooks

Similar questions

Calculate the molarity of AgNO3 in a solution prepared by dissolving 1.44 g AgNO3 in enough water to form 1.00 L solution.
87. What volume of 0.151 N NaOH is required to neutralize 24.2 mL of 0.125 N H2SO4? What volume of 0.151 N NaOH is required to neutralize 24.2 n1L of 0.125 M H2SO4?
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
How would you prepare from the solid and pure water (a) 0.400 L of 0.155 M Sr(OH)2? (b) 1.75 L of 0.333 M (NH4)2CO3?
Silver ions can be found in some of the city water piped into homes. The average concentration of silver ions in city water is 0.028 ppm. (a) How many milligrams of silver ions would you ingest daily if you drank eight glasses (eight oz/glass) of city water daily? (b) How many liters of city water are required to recover 1.00 g of silver chemically?
If cobalt(II) sulfate is heated too strongly, the following reaction will occur CoSO4(s) à CoO(s) + SO3(g) If you are heating a sample of CoSO4·6H2O and this reaction occurs along withdehydration, what will happen to the experimental percent water? Explain your answer.
At sea level, there are approximately 2.6 × 1025 molecules m–3 of the atmosphere. There are 1.17 × 1022 molecules m–3 of one of the gases making up the atmosphere. What is the concentration of this gas as a proportion of the total number of molecules in the atmosphere, expressed in parts per million (ppm)?
What volume (in liters) of CO2 measured at STP would be produced if 22.6 mL of 3 M HCl reacted with an excess amount of sodium bicarbonate? NaHCO3(s) + HCl(aq) → NaCl(aq) + H2O(l) + CO2(g)
PCl3(g) + 3 NaF(s) PF3(g) + 3 NaCl(s) K = 9.78 x 1031If 12.56 g of NaF(s) and 17.89 g of NaCl(s) are added to a 1.40 L container containing 26.67 g of PCl3(g), calculate theequilibrium concentrations of each gas.
What is the molarity of C6H12O6 in an aqueous solution that is prepared by dissolving a 25.91 g sample of impure C6H1206 in water to make 575.0 mL of solution. Assume that the sample is 81.0% C6H12O6 by mass. Enter your answer in mol L-1, accurate to three significant figures. Do not include units as part of your answer. Use the following molar masses, in g mol-1, for your calculations. H, 1.008 C, 12.01 O, 16.00
1. When potassium dichromate (K2CRO4) is added to a solution containing 0.500 g silver nitrate (AGNO3), solid silver chromate (Ag2CrO4) is formed. ( Note: Be sure to write down the balanced chemical equation.) a) Determine the theoretical yield of the silver chromate precipitate. b) If 0.455 g of silver chromate is obtained, calculate the percentage yield.
About 6x 10°g of goldis thought to be dissolved in the oceans of the world. If the total volume of the oceans is 1.5 x 1021 L, what is the average molar concentration of gold in seawater?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

What is the volume of CO2 gas produced at a pressure of 645 torr and a temperature of 800 K when 45.0 g of calcium carbonate (CaCO3, molar mass = 100.1 g/mol) decomposes completely according to the following reaction? CaCO →→CaO(s) + CO2(g) a) 34.8 L b) 30.9 L c) 27.1 L d) 23.2 L e) 19.3 L