/yb2 841.945 37 0 obj /MediaBox [0 0 595 842] /Filter /FlateDecode /yb1 0.055 /Type /Page /yt1 0.055 /MediaBox [0 0 595 842] /Producer (SAMBox 1.0.47.RELEASE \(www.sejda.org\)) /MediaBox [0 0 595 842] << stream Write the chemical equation for the formation of CO 2. << /TrimBox [0 0.055 595 841.945] << 1 0 obj /Rotate 0 /Resources 82 0 R /BleedBox [0 0.055 595 841.945] /TrimBox [0 0.055 595 841.945] << /yt1 0.055 /u2pMat [1 0 0 -1 0 842] /ProcSet [/PDF /Text /ImageB] /TrimBox [0 0.055 595 841.945] /Rotate 0 /yt2 841.945 /xt2 595 Standard molar heat enthalpy (H ∘) of a compound is equal to its standard heat of formation from most stable states of initial components. >> /CropBox [0 0 595 842] /Tabs /S /xt1 0 16 0 obj /Parent 3 0 R /yb2 841.945 /yt1 0.055 /yt2 841.945 /Resources 62 0 R >> /yb2 841.945 /yt2 841.945 /u2pMat [1 0 0 -1 0 842] /yb1 0.055 /xb2 595 /MediaBox [0 0 595 842] /Parent 3 0 R /u2pMat [1 0 0 -1 0 842] /Rotate 0 /Contents 51 0 R /BleedBox [0 0 595.32 841.92] /Resources 84 0 R /xt2 595 /u2pMat [1 0 0 -1 0 842] Enthalpy of formation (ΔHf) is the enthalpy change for the formation of 1 mol of a compound from its component elements, such as the formation of carbon dioxide from carbon and oxygen. /xb1 0 with most equations. /Parent 3 0 R endobj /u2pMat [1 0 0 -1 0 842] /u2pMat [1 0 0 -1 0 842] /Resources 88 0 R /Resources 41 0 R /yb1 0.055 Standard Enthalpy of Formation* for Atomic and Molecular Ions Cations ΔH˚ f (kJ/mol) Cations ΔH˚ f (kJ/mol) Anions ΔH˚ f (kJ/mol) Anions ΔH˚ f (kJ/mol) Ag+(aq) +105.9 K+(aq) −251.2 Br−(aq) −120.9 H 2PO 4 −(aq) −1302.5 Al3+(aq) −524.7 Li+(aq) −278.5 Cl−(aq) −167.4 HPO 4 2−(aq) −1298.7 Ba2+(aq) −538.4 Mg2+(aq) −462.0 ClO endobj /Type /Page 20 0 obj /MediaBox [0 0 595 842] /MediaBox [0 0 595 842] >> /xb1 0 endobj /yt1 0.055 /CropBox [0 0 595 842] /yt2 841.945 �"��L�RX,Y��Դ�~�e&�r��=o�ŊyW��],$�� G���x�ؓ�tM�_�0�.�����Mf�P:PJLI6abIE�$4���|�ݚw�r�]�]����,�SY�V2�*�w�n�A����̈́������]|� T�[*y���յ}�� ����I[Kr0T�(H#�R��BJ� �0,4Z/kZ�[گg�*)�8b�Y^ﶛٴ��C5��-S—p�yؚuW������C�j\P�"%KM��BK���:�O�d;�����T���4-�7��<8��f�i'B�!|*��44�} S�'Y>���(a�C�� �uZ�� [��ْcA������)N�F�"RS1-`�E`;;���b9��[�fI�j7ʋ���ݏ"��G2_'��|6�ݭg��8n�zWm��TKzh�~�K>��k�:R2���Y=�-+/�?Lr�0x* S��6�mh�P���y�s���. /CropBox [0 0 595 842] /BleedBox [0 0.055 595 841.945] /xt1 0 /Type /Page /LastModified (D:20170501153736+01'00') /Rotate 0 /yt2 841.945 /TrimBox [0 0.055 595 841.945] /xt2 595 Calculate the heat of formation of propane gas... Standard Enthalpy of Formation: Explanation & Calculations, Hess's Law: Definition, Formula & Examples, Acid-Base Buffers: Calculating the pH of a Buffered Solution, Rate of a Chemical Reaction: Modifying Factors, Determining Rate Equation, Rate Law Constant & Reaction Order from Experimental Data, Bond Enthalpy: Definition, Calculations & Values, Lewis Structures: Single, Double & Triple Bonds, The Common Ion Effect and Selective Precipitation, Calculating Molarity and Molality Concentration, Bronsted-Lowry Acid: Definition & Examples, What is a Calorimeter? /xb1 0 >> /yt1 0.055 /Parent 3 0 R /TrimBox [0 0.055 595 841.945] /Contents 61 0 R >> endobj /yt1 0.055 Note that the table for Alkanes contains Δ f H o values in kcal/mol (1 kcal/mol = 4.184 kJ/mol), and the table for Miscellaneous Compounds and Elements contains these values in kJ/mol. /Resources 48 0 R /xt1 0 [], and was also used for the initial development of high-accuracy ANLn composite electronic structure methods []. /u2pMat [1 0 0 -1 0 842] /xb2 595 /MediaBox [0 0 595 842] /yb2 841.945 /u2pMat [1 0 0 -1 0 842] /Parent 3 0 R O2(g) is in all 3 equations. /yt2 841.945 /xb2 595 /yt2 841.945 /Contents 79 0 R /u2pMat [1 0 0 -1 0 842] /Contents 69 0 R /Contents 85 0 R /MediaBox [0 0 595 842]

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