{"id":14701,"date":"2023-04-19T10:00:29","date_gmt":"2023-04-19T04:30:29","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=14701"},"modified":"2023-04-20T09:53:20","modified_gmt":"2023-04-20T04:23:20","slug":"energy-released-bond-formed","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/energy-released-bond-formed\/","title":{"rendered":"Why is energy released when a bond is formed?"},"content":{"rendered":"
<\/p>\n
People also ask<\/strong><\/p>\n Formation of hydrogen bromide, HBr :<\/strong><\/span><\/p>\n H2<\/sub>(g) + Br2<\/sub>(g) \u2192\u00a02HBr(g) Decomposition of ammonia:<\/strong><\/span><\/p>\n <\/p>\n Example:\u00a0<\/strong>The following is the chemical equation of the formation of hydrogen chloride. <\/p>\n","protected":false},"excerpt":{"rendered":" Why is energy released when a bond is formed? Energy change during formation and breaking of bonds During a chemical reaction, the bonds between the atoms in the reactans need to be broken first before new bonds between the atoms in the products can be formed. Chemical reactions involve bond breaking and bond formation: […]<\/p>\n","protected":false},"author":3,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_genesis_hide_title":false,"_genesis_hide_breadcrumbs":false,"_genesis_hide_singular_image":false,"_genesis_hide_footer_widgets":false,"_genesis_custom_body_class":"","_genesis_custom_post_class":"","_genesis_layout":"","footnotes":""},"categories":[84],"tags":[5761,5760,5763,5762,5759,5758,5757],"yoast_head":"\n\n
\n<\/a><\/li>\n
\nH – H + Br – Br \u2192\u00a02 H – Br<\/p>\n\n
\nEb\u00a0<\/sub>= energy to break 1 mole of H – H bonds + energy to break 1 mole of Br – Br bonds
\n= 436 kJ + 192 kj = 628 kJ<\/li>\n
\nEf\u00a0<\/sub>= energy to form 2 moles of H – Br
\n= 2 x 366 kJ = 732 kJ<\/li>\n
\n\u0394H = Eb<\/sub> – Ef
\n<\/sub>= 628 kJ – 732 kJ = -104 kJ<\/li>\n
\nH2<\/sub>(g) + Br2<\/sub>(g) \u2192 2HBr(g) \u00a0 \u00a0\u0394H = -104 kJ<\/li>\n
\n<\/li>\n<\/ul>\n\n
\nEb\u00a0<\/sub>= energy to break 6 moles of H – N bonds
\n= 6 x 391 kJ = 2346 kJ<\/li>\n
\n
\n<\/sub><\/li>\n
\n\u0394H = Eb<\/sub>-Ef<\/sub>
\n<\/sub>= 2346 kJ – 2254 kJ = +92 kJ
\nThe decomposition of ammonia to form nitrogen and hydrogen is an endothermic reaction.
\n2NH3<\/sub>(g) \u2192 N2<\/sub>(g) + 3H2<\/sub>(g) \u00a0 \u00a0\u0394H = +92 kJ<\/li>\n
\n<\/li>\n<\/ul>\n
\nH2<\/sub>(g) + Cl2<\/sub>(g) \u2192\u00a02HCl(g)
\nCalculate the overall heat change in the reaction.
\nGiven that the bond energy of H – H = 436 kJ mol-1<\/sup>, Cl – Cl = 242 kJ mol-1<\/sup>, H – Cl = 432 kJ mol-1<\/sup>.
\nSolution:<\/strong><\/p>\n