Gas Stoichionmetry1. What volume (in mL) of carbon dioxide forms when 525 milligrams of calcium carbonate reacts with excesshydrochloric acid? Assume that the carbon dioxide is formed at a pressure of 201 kPa and a temperature of 25°C.CaCO3(5) + HClaq) → CO,(g) + H,0,g) + CaClz{aq}[unbalanced equation]metalஅ

The volume of carbon dioxide is to be calculated when 525 milligrams of calcium carbonate reacts…

Answered: Gas Stoichionmetry 1. What volume (in…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter8: Properties Of Gases

Section: Chapter Questions

Problem 129QRT

See similar textbooks

Similar questions

5-39 An 8.00-g sample of a gas occupies 22.4 L at 2.00 atm and 273 K. What is the molar mass of the gas?
5-107 If 60.0 g of NH3 occupies 35.1 L under a pressure of 77.2 in. Hg, what is the temperature of the gas, in °C?
While ethanol CH3CH2OH is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene CH2CH2 with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 200.mL flask with 1.2atm of ethylene gas and 1.3atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.25atm of ethylene gas and 0.35atm of water vapor. The engineer then adds another 0.30atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.
(References) An 18.6 mL volume of hydrochloric acid reacts completely with a solid sample of MgCO3. The reaction is 2HC1(aq)+MgCO,(s)CO2(9) + H,O(1) + MgCl, (aq) The volume of CO2 formed is 175 mL at 23°C and 731 mmHg. What is the molarity of the HCl solution? Molarity- Submit Answer Try Another Version 3 item attempts remaining pr pt
(ans: -7.50 x 10 ) one mole of sucrose). Imol %3D 9reaction=n AH %3D %3D (ans: -5.64 x 10 kJ/mol) Calcium chloride and sodium hydroxide react according to the equation: CaCl(aq) + 2 NaOH(aq) → Ca(OH),(s) +2 NaCl(aq) What volume of 2.00 M NaOH would be needed to react with 50.0 mL of 1.50 M CaCl,? a, 017 (ans: 75.0 mL) b) When 50.0 mL of 1.50 M CaCl, solution and 80.0 mL of 2.00 M NAOH solution (i.e., 5.0 mL more than calculated in part (a)) both initially at 22.3°C are mixed in a coffee-cup calorimeter with a calorimeter constant of 12.8 J/ C, the temperature fell to 20.0°C. If the density of the reaction mixture is 1.03 g/mL and its specific heat 3.94 J/g°C, calculate the heat absorbed hv the reaction. (ans: 1.24 x 103) c) Calculate AH (in kJ per mole of Ca(OH)2 formed) for the reaction. (ans: 1.6 x 10' kJ/mol)
I’m confused to find the grams that are decomposed and how to tell what atom is oxidized
What is the Qc for the following reaction, if a mixture contains gases with the following concentrations: CH4, 26 M; H2O, 24 M; CO, 26 M; H2 15 M, at a temperature of 760 0C? CH4(g) + H2O(g) CO(g) + 3H2(g)
n Unknown elemental metal was reacted with Hydrochloric Acid. It was determined that this reaction evolved Hydrogen gas and left the metal in solution in the 2+ oxidation state. The Unknown metal was then subjected to the same test as Magnesium in the “Molar Mass of Magnesium” lab. After some adjustments to get the volume of gas collected in the right range, the following results were obtained: Mass of Metal used = 0.3682 g P (atmospheric) = 761.1 mm Hg Temperature of gas = 21.6 degrees C Volume of gas collected = 67.5 ml Difference in height of solution levels in the buret and beaker = 163.0mm Vapour pressure of H20 at gas temperature = 19.349 mm Hg Some Constants: R = 0.0820575 L*Atm/mol/K = 62.3637 L*mmHg/mol/K dsolution = 1.00g/ml dHg = 13.6 g/ml From this data, calculate and report the molar mass of the unknown metal with correct significant figures and unit
Explain in terms of the Kinetic Molecular Theory the following situations: a) Why does compressing a gas raise the temperature of the system? b) Explain why the density of a gas is so much lower than the density of its liquid form? c) Explain in detail the dissolving process of KCl in water. d) Explain why the solid precipitate AGl (s) forms when solutions of KCl (aq) and AgNO3 (aq) are mixed.
ezto.mheducation.com/ext/map/index.html?_con3con&external_browser=0&launchUrl=https%25 pter 19 Sa Enter your answer in the provided box. Given the following data, ts 2H9²*(aq) + 2e→ Hg,“(aq) E = 0.92 V eBook Hg,"(aq) + 2e¯ → 2Hg(l) E = 0.85 V ferences calculate AG for the following process at 25°C: Hg,"(aq) → Hg²*(aq) + Hg(1) kJ / mol raw < Prev e here to search 2.
Stoichiometry with Partial Pressure Gas jar Gas collects here Trough of water Bee hive shelf Reaction mixture 2 KCIO, 3(s) + > 2 KCI (s), 30 2(g) A sample of KCIO3 is partially decomposed by heating, producing O2 gas that is collected safely over water. The volume of total gas collected is 2.50 x 10-4 m³ at 26 °C, giving 101.99 kPa total pressure. How many grams of KCIO3 were decomposed? What atom was oxidized? What atom was reduced? The pressure of water vapor at 26 °C is 25 torr. SHOW ALL WORK!
For the reaction: 2 SO2(g) + O2(g) vessel is filled with these gases, such that [SO2] = 6.0 M, [O2] = 6.0 M and [SO3] = =2 SO3(g), Kc = 6.9 × 1024 at 25°C. If a reaction %3D 6.0 M, in which direction will the reaction proceed? The reaction proceeds to the right. The reaction is already at equilibrium. The reaction volume must be specified to answer this question. The value of Kp must be specified to answer this question. The reaction proceeds to the left.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Introduction to General, Organic and Biochemistry

Chemistry

ISBN:

9781285869759

Author:

Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Introduction to General, Organic and Biochemistry

Chemistry

ISBN:

9781285869759

Author:

Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS