The following reaction for dissolution of limestone by reaction with carbon dioxide and water is geochemically...
The following reaction for dissolution of limestone by reaction with carbon dioxide and water is geochemically important.
CaCO3 (calcite) + H2CO3 <????> Ca2+ + 2HCO?3
(a) Calculate the standard free energy change and the enthalpy change for the reaction at 25?C and 1 atm total pressure.
(b) Calculate the equilibrium constant at 25?C and 1 atm total pressure.
(c) Will an increase in temperature favor a shift toward products or reactants for this reaction?
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The following reaction for dissolution of limestone by reaction
with carbon dioxide and water is geochemically...
The reaction between lime (CaO(s)) and carbon dioxide (CO2(g)) forms the predominant mineral in limestone, CaCO3(s),...
The reaction between lime (CaO(s)) and carbon dioxide (CO2(g)) forms the predominant mineral in limestone, CaCO3(s), (Delta Hrxn° = −177.1 kJ/mol, Delta Srxn° = −158.2 J/K∙mol). Lime is a key component in making concrete and is made from limestone. What is the minimum temperature required to shift the equilibrium toward lime (CaO(s)) from limestone (CaCO3(s))?
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas....
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete the lime absorbs CO, from the air and turns back into hard, durable limestone Suppose a limekiln of volume 350. L is pressurized with carbon dioxide gas to 5.60 atm, and heated to 1110. °C. When the amount of CO2 has...
Acid precipitation dripping on limestone produces carbon dioxide by the following reaction: CaCO3(s) + 2H+ (aq)...
Acid precipitation dripping on limestone produces carbon dioxide by the following reaction: CaCO3(s) + 2H+ (aq) —— Ca2+ (aq) + CO2(g) +H20(1) 17.0 mL of CO2 was produced at 25.0°C and768.0 mm Hg. Part 1 (1 pt) W See Periodic Table D See Hint How many moles of CO2 were produced? 78.6 mol Part 2 (1 pt) D See Hint How many milligrams of CaCO3 were consumed? 7.86 mg
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas....
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete — the lime absorbs CO2 from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 750.L and heated to 770.0°C When the amount of CaCO3 has stopped changing, it is...
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas....
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO2 from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 250. L and heated to 870.0 °C. When the amount of CaCO3 has stopped changing,...
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen...
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 500. mL flask at 20·°C with 4.9 atm of carbon monoxide gas and 2.5 atm of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains...
For the equilibrium reaction of carbon dioxide with water, what is the appropriate reaction equation? A)...
For the equilibrium reaction of carbon dioxide with water, what is the appropriate reaction equation? A) H2O + CO2 HCO3 B) H2O + CO2 H2CO2 C) H2O + CO H2CO3 D) H2O +2CO2 H2CO3 E) H2O + CO2 H2CO3
please help 10. What effect do the listed changes have on the position of the equilibrium in the reaction of carbon...
please help
10. What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen? C + 2How → CHILE AH -18 kcal/mol (-75 kd/mol) A. Increasing temperature: A increasing the temperature shifts the equilibrium to the right, favoring, product B. Increasing the temperature shifts the equilibrium to the left, favoring reactants. B. Increasing pressure by decreasing volume: A B. Increasing the pressure shifts the equilibrium to the left, favoring reactants Increasing...
For the dissolution of thenardite shown below, calculate the following (at STP, 25 °C and 1...
For the dissolution of thenardite shown below, calculate the following (at STP, 25 °C and 1 atm):Na2SO4 (s) ↔ 2Na+(aq) + SO42-(aq) (a) standard??° enthalpy of reaction (∆????°), ??° (b) standard Gibbs free energy of reaction (∆?? ) using standard Gibbs free energy of formation values (∆?? ), and (c) equilibrium constant (K). (d) Is this a spontaneous reaction [i.e., the dissolution reaction (left to right)]? Explain.
answer both parts 1 and 2 Acid precipitation dripping on limestone produces carbon dioxide by the...
answer both parts 1 and 2
Acid precipitation dripping on limestone produces carbon dioxide by the following reaction: CaCO3(s) + 2H+ (aq) —— Ca²+ (aq) + CO2(g) +H20(1) 19.5 mL of CO2 was produced at 25.0°C and779.0 mm Hg. Part 1 (1.5 points) How many moles of CO2 were produced? mol Part 2 (1.5 points) How many milligrams of CaCO3 were consumed? mg
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete the lime absorbs CO, from the air and turns back into hard, durable limestone Suppose a limekiln of volume 350. L is pressurized with carbon dioxide gas to 5.60 atm, and heated to 1110. °C. When the amount of CO2 has...
Acid precipitation dripping on limestone produces carbon dioxide by the following reaction: CaCO3(s) + 2H+ (aq) —— Ca2+ (aq) + CO2(g) +H20(1) 17.0 mL of CO2 was produced at 25.0°C and768.0 mm Hg. Part 1 (1 pt) W See Periodic Table D See Hint How many moles of CO2 were produced? 78.6 mol Part 2 (1 pt) D See Hint How many milligrams of CaCO3 were consumed? 7.86 mg
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO2 from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 250. L and heated to 870.0 °C. When the amount of CaCO3 has stopped changing,...
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 500. mL flask at 20·°C with 4.9 atm of carbon monoxide gas and 2.5 atm of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains...
please help
10. What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen? C + 2How → CHILE AH -18 kcal/mol (-75 kd/mol) A. Increasing temperature: A increasing the temperature shifts the equilibrium to the right, favoring, product B. Increasing the temperature shifts the equilibrium to the left, favoring reactants. B. Increasing pressure by decreasing volume: A B. Increasing the pressure shifts the equilibrium to the left, favoring reactants Increasing...
answer both parts 1 and 2
Acid precipitation dripping on limestone produces carbon dioxide by the following reaction: CaCO3(s) + 2H+ (aq) —— Ca²+ (aq) + CO2(g) +H20(1) 19.5 mL of CO2 was produced at 25.0°C and779.0 mm Hg. Part 1 (1.5 points) How many moles of CO2 were produced? mol Part 2 (1.5 points) How many milligrams of CaCO3 were consumed? mg
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