Given the following standard enthalpy change, use the standard enthalpies of formation in Table 5.3 to calculate the standard enthalpy of formation of CuO(s): CuO(s) + H2(8) – Cu(s) + H2O(1) AH = -129.7k) %3D
Given the following standard enthalpy change, use the standard enthalpies of formation in Table 5.3 to calculate the standard enthalpy of formation of CuO(s): CuO(s) + H2(8) – Cu(s) + H2O(1) AH = -129.7k) %3D
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section4.11: Fuels For Society And Our Bodies
Problem 4.19CE: Correlate the fuel values and caloric values calculated in Problem-Solving Example 4.15 with the...
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Transcribed Image Text:**TABLE 5.3: Standard Enthalpies of Formation, ΔH⁰ₒ, at 298 K**
| Substance | Formula | ΔH⁰ₒ (kJ/mol) |
|---------------------|-------------|---------------|
| Acetylene | C₂H₂(g) | 226.7 |
| Ammonia | NH₃(g) | -46.19 |
| Benzene | C₆H₆(l) | 49.0 |
| Calcium carbonate | CaCO₃(s) | -1207.1 |
| Calcium oxide | CaO(s) | -635.5 |
| Carbon dioxide | CO₂(g) | -393.5 |
| Carbon monoxide | CO(g) | -110.5 |
| Diamond | C(s) | 1.88 |
| Ethane | C₂H₆(g) | -84.68 |
| Ethanol | C₂H₅OH(l) | -277.7 |
| Ethylene | C₂H₄(g) | 52.30 |
| Glucose | C₆H₁₂O₆(s) | -1273 |
| Hydrogen bromide | HBr(g) | -36.23 |
| Hydrogen chloride | HCl(g) | -92.30 |
| Hydrogen fluoride | HF(g) | -268.60 |
| Hydrogen iodide | HI(g) | 25.9 |
| Methane | CH₄(g) | -74.80 |
| Methanol | CH₃OH(l) | -238.6 |
| Propane | C₃H₈(g) | -103.85 |
| Silver chloride | AgCl(s) | -127.0 |
| Sodium bicarbonate | NaHCO₃(s) | -947.7 |
| Sodium carbonate | Na₂CO₃(s) | -1130.9 |
| Sodium chloride | NaCl(s) | -410.9 |
| Sucrose | C₁₂H₂₂O
![**Practice Exercise 2**
Given the following standard enthalpy change, use the standard enthalpies of formation in Table 5.3 to calculate the standard enthalpy of formation of CuO(s):
\[ \text{CuO(s) + H}_2\text{(g) → Cu(s) + H}_2\text{O(l)} \]
\[ \Delta H^\circ = -129.7 \text{ kJ} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F90b2ad7e-71be-4993-92e0-fe2030354ee3%2F0487714a-2f03-4b25-a743-2095943300ba%2F41gjgfh_processed.png&w=3840&q=75)
Transcribed Image Text:**Practice Exercise 2**
Given the following standard enthalpy change, use the standard enthalpies of formation in Table 5.3 to calculate the standard enthalpy of formation of CuO(s):
\[ \text{CuO(s) + H}_2\text{(g) → Cu(s) + H}_2\text{O(l)} \]
\[ \Delta H^\circ = -129.7 \text{ kJ} \]
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