WebOct 7, 2024 · calculate molar enthalpy. Using the equations. 2 H₂ (g) + O₂ (g) → 2 H₂O (l) ∆H° = -572 kJ/mol. Ca (s) + ½ O₂ (g) → CaO (s) ∆H° = -635 kJ/mol. CaO (s) + H₂O (l) → Ca (OH)₂ (s) ∆H° = -64 kJ/mol. Determine the molar enthalpy (in kJ/mol) for the reaction Ca (s) + 2 H₂O (l) → Ca (OH)₂ (s) + H₂ (g). Follow • 2. WebNov 4, 2024 · The fact that is is the reverse, means we must change the sign of ∆H, thus making it positive. So, at this point it would be +635 kJ/mole. Now, since we doubled the …
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http://www.1010jiajiao.com/gzhx/shiti_id_6a318b42f8f701ecc19c7743de082f08 WebJun 30, 2024 · The enthalpy of decomposition is 656.3 KJ/mol. Given that the enthalpy of decomposition is obtained from; ΔHrxn = ∑ΔHf(products) - ∑ΔHf(reactants) ... the species involved in the reaction are; ΔHf(CaO)(s)) = -157.3 KJ/mol. ΔHf((CO2)(g)) =-393.5 KJ/mol. ΔHf(CaCO3)(s)) = -1207.1 KJ/mol. Substituting values; ΔHrxn = 656.3 KJ/mol. Learn ... car belts names
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WebGiven that CaO(s) + H 2 O(l) → Ca(OH) 2 (s), ΔH o rxn = -64.8 kJ/mol, how many grams of CaO must react in order to liberate 525 kJ of heat? Expert Answer. Who are the experts? Experts are tested by Chegg as specialists in their subject area. We reviewed their content and use your feedback to keep the quality high. WebApr 15, 2024 · DH°f [CaCO3(s)] = –1206.9 kJ/mol; DH°f [CaO(s)] = –635.1 kJ/mol; DH°f [CO2(g)] = –393.5 kJ/mol CaCO3(s) --> CaO(s) + CO2(g) See answers Advertisement Advertisement jufsanabriasa jufsanabriasa Answer: Explanation: Using Hess's law, you can obtain ΔHrxn from ΔHf of products and reactants, thus: http://www.endmemo.com/chem/compound/cao.php car belt slipping repair