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thermochemistry and rate of reactions, CH4(g)+2O2(g)-->CO2(g)+2H2O(g),…

- - - - =carbon dioxide and water vapour
- - - - few exothermic reactions are totally spontaneus at normal temperatures
        
        energy usually needed
        
        when fuel is burnt, energy needed to ignite(like a spark, a match or sunlight)
      - some bonds must be broken befour a reaction happens
- - - - -
        
        CO2(g)+2H2O(g)
      - heat given out, exothermic(opposite if heat taken in, endothermic)
        
        because bonds CO2 H2O stronger than CH4 O2(products more stable than reactants
        
        endothermic ractions far less common
        
        fuel burnt in car engines
        
        N2(g)+O2(g)-->2NO(g)
        
        nitrogen+oxygen-->nitrogen monoxide
        
        A negative ΔH releasing energy(exothermic), a positive ΔH ganing energy(endothermic)