Chemistry Enthalpy

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ΔH value in an endothermic reaction is a positive number.

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True

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What type of reaction is shown in the reaction pathway?

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exothermic reaction

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How do you calculate Enthalpy of a reaction?

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ΔH = ΔH_products - ΔH_reactants

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Calculate the enthalpy of the reaction: Ca(OH)₂ -> CaO + H₂O
ΔHf in kJ/mol:  
      Ca(OH)₂  -983.2
        CaO         -634.9
        H₂O         -285.5

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62.8 kJ

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Using the equations below:
C_(s) + O_2(g) → CO_2(g) ∆H = –390 kJ Mn_(s) + O_2(g) → MnO_2(s) ∆H = –520 kJ
what is ∆H (in kJ) for the following reaction?
MnO_2(s) + C_(s) → Mn_(s) + CO_2(g)

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130

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What is the ∆H value (in kJ) for the reaction: MgO_(s) + H_2(g) → Mg_(s) + H₂O_(g) given the following equations: Mg_(s) + O_2(g) → MgO_(s) ∆H = –602 kJ H_2(g) + O_2(g) → H₂O_(g) ∆H = –242 kJ

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+360

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Calculate the enthalpy change for the reaction: H_{2 (g)} + CO_{2 (g)} → HCOOH _(l) given that the standard enthalpy changes of formation of carbon dioxide and methanoic acid are −394 kJ/mol and −409 kJ/mol respectively.

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−15 kJ/mol

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The standard enthalpy change for the combustion of graphite is −393.5 kJ/mol and that of diamond is −395.4 kJ/mol.
What is the enthalpy change for the reaction below, in kJ/mol? C _{(s, graphite)} → C _{(s, diamond)}

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−1.9 kJ/mol

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endothermic reaction

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Calculate ΔH_rxn for the reaction: CO_2(g) + N_2(g) ⟶ NO_(g) + CO_(g) using the following data: CO(g) -110 kJ/mol CO2(g) -394 kJ/mol NO(g) 90 kJ/mol

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374 kJ/mol