Carbon dioxide reacts with calcium hydroxide according to the following reaction: CO2(g) +Ca(OH)2 (aq) = CaCo(s)...

Carbon dioxide reacts with calcium hydroxide according to the following reaction: CO2(g) +Ca(OH)2 (aq) = CaCo(s) + H2O(l) a 5.0 L container contains 1.0 L Ca(OH)2 solution. CO2 (g) is introduced to the container. At the beginning the CO2 pressure is 4.0 atm. When the reaction is complete, the pressure drops to zero. The temperature is 298K. Assume CO2 behaves as an ideal gas. From this information calculate 1) the extent of the reaction, and 2) the number of grams CaCO3 (s) formed

Expert Solution

1)
Since all of CO2 has reacted, the reaction is fully complete
Hence the extent of the reaction is 100 % complete.

2)
Lets calculate the number of moles of CO2 present initially.
Volume occupied by CO2 = 4 L

usE:
P*V = n*R*T
4 atm * 4 L = n * 0.0821 atm L/mol-K * 298
n = 0.654 mol

So, 0.654 mol of CO2 has reacted.

From the reaction:
CO2(g) +Ca(OH)2 (aq) = CaCo3(s) + H2O(l)
1 mol of CO2 gives 1 mol of CaCO3.
So, number of moles of CaCo3 formed = 0.654 mol
Molar mass of CaCo3= 100 g/mol
So,
mass of CaCo3 formed = number of moles * molar mass
= 0.654 * 100
= 65.4 g
Answer: 65.4 g

queen_honey_blossom answered 1 year ago

Ca(s) reacts with water forming calcium hydroxide. If a 3.00 g chunk of calcium is reacted...

Ca(s) reacts with water forming calcium hydroxide. If a 3.00 g chunk of calcium is reacted with water and the solution is further diluted with water to a volume of 250 mL at 60.0 °C (d = 0.981 g/mL) calculate the following: a) the concentration of calcium hydroxide b) the concentration of hydroxide anions c) the molality of calcium hydroxide d) the molality of hydroxide anions e) the mole fraction of calcium hydroxide f) the mole fraction of hydroxide anions...

Calcium hydride, CaH2, reacts with water to form hydrogen gas: CaH2(s)+2H2O(l)→Ca(OH)2(aq)+2H2(g) This reaction is sometimes used...

Calcium hydride, CaH2, reacts with water to form hydrogen gas: CaH2(s)+2H2O(l)→Ca(OH)2(aq)+2H2(g) This reaction is sometimes used to inflate life rafts, weather balloons, and the like, where a simple, compact means of generating H2 is desired. Part A How many grams of CaH2 are needed to generate 146 L of H2 gas if the pressure of H2 is 824 torr at 22 ∘C? The metabolic oxidation of glucose, C6H12O6, in our bodies produces CO2, which is expelled from our lungs as...

Consider the dissolution of calcium hydroxide: Ca(OH)2(s) --> Ca2+(aq) + 2OH‑(aq) K = 4.7 x 10‑6...

Consider the dissolution of calcium hydroxide: Ca(OH)2(s) --> Ca2+(aq) + 2OH‑(aq) K = 4.7 x 10‑6 Write the equilibrium expression for this reaction. 2. Identify whether the following actions would favor the formation of products, reactants, or have no affect upon the dissolution of calcium hydroxide. Explain each answer. a. Addition of CaCO3 to an equilibrium mixture of calcium hydroxide and water. b. Addition of Na2CO3 to an equilibrium mixture of calcium hydroxide and water. c. Addition of HCl to...

Consider this reaction between solid carbon and carbon dioxide gas. C(s) + CO2(g) ⇌ 2 CO(g);...

Consider this reaction between solid carbon and carbon dioxide gas. C(s) + CO2(g) ⇌ 2 CO(g); ΔH = +172.5 kJ/mol Please explain the following: When chemical systems are subjected to stresses, the equilibrium position may shift toward the reactants or products, or it may be unaffected. How would each of the following changes affect this equilibrium? 1. decreasing the temp 2. increasing the CO2 3. increasing the volume of the container 4. adding C 5. adding a catlyst Options: Would...

Calcium carbonate decomposes to form calcium oxide and carbon dioxide, like this: CaCO3(s)→CaO(s)+CO2(g) At a certain...

Calcium carbonate decomposes to form calcium oxide and carbon dioxide, like this: CaCO3(s)→CaO(s)+CO2(g) At a certain temperature, a chemist finds that a 9.0L reaction vessel containing a mixture of calcium carbonate, calcium oxide, and carbon dioxide at equilibrium has the following composition: Compound Amount CaCO3 25.3 g CaO 14.9 g CO2 33.7 g Calculate the value of the equilibrium constant Kc for this reaction. Round your answer to 2 significant digits.

When calcium carbonate is added to hydrochloric acid, carbon dioxide, and water are produced. CaCO3(s)+2HCl(aq)--->CaCl2(aq)+H2O(l)+CO2(g) a....

When calcium carbonate is added to hydrochloric acid, carbon dioxide, and water are produced. CaCO3(s)+2HCl(aq)--->CaCl2(aq)+H2O(l)+CO2(g) a. How many grams of calcium chloride will be produced when 27.0g of calcium carbonate are combined with 12.0g of hydrochloric acid? 2. Which reactant is excess and how many grams of this reactant will remain after the reaction is complete?

For the reaction Ca(OH)2(s)+2HCl(aq)→CaCl2(aq)+2H2O(l) a) How many grams of Ca(OH)2 are required to react completely with...

For the reaction Ca(OH)2(s)+2HCl(aq)→CaCl2(aq)+2H2O(l) a) How many grams of Ca(OH)2 are required to react completely with 430 mL of 0.450 M HCl? b) How many kilograms of Ca(OH)2 are required to react with 333 L of a HCl solution that is 24.28% HCl by mass, and has a density of 1.12g/mL?

1. When heated, calcium carbonate gives off CO2 according to the following reaction: CaCO3(s) → CO2(g)...

1. When heated, calcium carbonate gives off CO2 according to the following reaction: CaCO3(s) → CO2(g) + CaO(s) You perform this reaction in lab by heating a test tube containing CaCO3 and collect the CO2 over water for later analysis. You collect 20.3 mL of gas. What mass of CO2 have you collected? Assume the temperature and pressure of your lab is 25 °C and 1.00 atm. The vapor pressure of water at 25 °C is 24.0 Torr. (a) 35.4...

What evidence indicates that Calcium Hydroxide (Ca(OH) 2 ) is a strong base?

Ca(s)+2H(aq)--> Ca^2+(aq)+H2 ∆H= -543 KJ/mol CaCO3(s)+2H(aq)-->Ca^2+(aq)+CO2(g)+H2O(l) ∆H= -15 KJ/mol Look up the heats formation for CO2...

Ca(s)+2H(aq)--> Ca^2+(aq)+H2 ∆H= -543 KJ/mol CaCO3(s)+2H(aq)-->Ca^2+(aq)+CO2(g)+H2O(l) ∆H= -15 KJ/mol Look up the heats formation for CO2 and H2O in the thermodynamic tables and use this information along with the above heats of reaction to calculate the standard enthalpy of formation for CaCO3. Write the balanced equations for the two heat of formations reactions, and use Hess Law in order to answer this question.

Question