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.

Expert Solution

C(s) + O2 (g) ------------> CO2(g) ∆H = -393.5Kj/mole

H2 + 1/2 O2(g) ----------> H2O (l) ∆H = -286 Kj/mole

--------------------------------------------------------------------------------------

C(s) + H2(g)+ 3/2 O2(g) -------------> CO2(g) + H2O(l) ∆H = -679.5KJ/mole

C(s)+ H2(g) + 3/2 O2(g) -------------> CO2(g) + H2O(l) ∆H = -679.5KJ/mole

Ca(s)+2H(aq)--> Ca^2+(aq)+H2 ∆H= -543 KJ/mol

----------------------------------------------------------------------------------------------

Ca(s) + C(s) +2H(aq) + 3/2 O2(g) -------------> Ca^2+ (aq) + CO2(g) + H2O(l) ∆H = -1222.5 KJ/mole

CaCO3(s)+2H(aq)-- ----------------------------> Ca^2+(aq)+CO2(g)+H2O(l) ∆H= -15 KJ/mol

(-) (-) (-) (-) (-) (-) (+)

--------------------------------------------------------------------------------------------------------------------------------------

Ca(s) + C(s) + 3/2 O2(g) --------------------> CaCO3(s) ∆H = -1207.5KJ/mole

queen_honey_blossom answered 1 year ago

1. The heats of formation of CO2(g) and H2O(l) are -394 and -285.8 kJ/mole, respectively. Using...

1. The heats of formation of CO2(g) and H2O(l) are -394 and -285.8 kJ/mole, respectively. Using the data for the following combustion reaction, calculate the heat of formation of C3H4(g). C3H4(g) + 4 O2(g) -> 3 CO2(g) + 2 H2O(l) DHo = -1,939.1 kJ 2. A 10.0 gram sample of CaO is dissolved in water in a calorimeter whose specific heat capacity is 4.37 kJ/K. The temperature decreases 2.70 K. Calculate the DHo for the following reaction. CaO(s) +...

C: CaCO3 (s) ----> CaO (s) + CO2 (g) delta H= +178 kJ/mol D: PCl3 (g)...

C: CaCO3 (s) ----> CaO (s) + CO2 (g) delta H= +178 kJ/mol D: PCl3 (g) + Cl2 (g) -----> PCl5 (g) delta H= - 88 kJ/mol Classify these changes as either LEFTWARD SHIFT, RIGTHWARD SHIFT, or NO SHIFT System C increase temperature System C decrease temperature System D increase temperature System D decrease temperature

For the following chemical equation: CaCO3(s) + 2HCl(aq).......>H2)(l) +CO2 (g) +CaCl2 (aq) A). How many liters...

For the following chemical equation: CaCO3(s) + 2HCl(aq).......>H2)(l) +CO2 (g) +CaCl2 (aq) A). How many liters of CO2 can form at STP when 18.5 mL of a 3.51 M HCl solution reacts with excess CaCO3? B). What is the molarity of a HCl solution if the reaction of 210 mL of the HCl solution with excess CaCO3 produces 12.1 L of CO2 gas at 725 mmHg and 18 C?

Classify the reaction Ca(OH)2 (aq) + H2CO3(aq) → CaCO3(s) + 2 H2O(l): a. Acid-Base b. Precipitation...

Classify the reaction Ca(OH)2 (aq) + H2CO3(aq) → CaCO3(s) + 2 H2O(l): a. Acid-Base b. Precipitation c. Both d. Neither Sodium phosphate reacts with calcium chloride. Write the balanced, net ionic equation, and then choose the coefficient associated with the calcium ion in that equation (choose 0 if not present): a. 0 b. 1 c. 2 d. 3 Sulfuric acid reacts with barium hydroxide. Write the balanced, net ionic equation, and then choose the coefficient associated with the hydroxide ion...

Consider the given reaction. MgCO3(s) + 2 HCl(aq) — MgCl2(aq) + H2O(l) + CO2(g)

Consider the given reaction. MgCO3(s) + 2 HCl(aq) — MgCl2(aq) + H2O(l) + CO2(g) Calculate the atom economy of this reaction to form carbon dioxide assuming that no other reactions are occurring. atom economy = _______ %

From the following heats of combustion, CH3OH(l) + 3/2O2(g) → CO2(g) + 2H2O(l) ΔHorxn= –726.4 kJ/mol...

From the following heats of combustion, CH3OH(l) + 3/2O2(g) → CO2(g) + 2H2O(l) ΔHorxn= –726.4 kJ/mol C(graphite) + O2(g) → CO2(g) ΔHorxn = –393.5 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔHorxn = –285.8 kJ/mol Calculate the enthalpy of formation of methanol (CH3OH) from its elements. C(graphite) + 2H2(g) + ½O2(g) → CH3OH(l)

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?

Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚...

Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚ for the reaction, given that: ∆Gf Zn(s) = 0, ∆Gf(H+) = 0, ∆Gf(H2) = 0, ∆Gf(Zn2+) = -147.1 kj/mol b) ∆G, when P(h2) = 750 mmHg, [Zn2+ aq] = 0.10 M, [H+] = 1.0 x 10^-4 M c) The pH when ∆G - -100 kJ, P(h2) = 0.922 atm, [Zn2+] = 0.200 M and the mass of Zn is 155 g.

Given the following balanced reaction, O2(g) + 4 H+(aq) + 4 Fe2+(aq) → 2 H2O(l) +...

Given the following balanced reaction, O2(g) + 4 H+(aq) + 4 Fe2+(aq) → 2 H2O(l) + 4 Fe3+(aq) What is the equilibrium constant (K)? The following information may be useful. O2(g) + 4 H+(aq) + 4e- → 2 H2O(l) Eº = 1.23 V Fe3+(aq) + e- → Fe2+(aq) Eº = 0.77 V

1. Determine ΔGo for the following reaction: 2 Na(s) + 2 H2O(l) --> H2(g) + 2...

1. Determine ΔGo for the following reaction: 2 Na(s) + 2 H2O(l) --> H2(g) + 2 OH-(aq) + 2 Na+(aq) 2. Calculate K for the oxidation of iron by H+: 2 Fe(s) + 6 H+(aq) --> 2 Fe3+(aq) + 3 H2(g)

Question