How much heat is produced when 2.63 g of phosphorous and 40g of Bromine is allowed to react according to following equation
`P_(4(s))+6Br_(2(l)) rarr 4PBr_(3(g)), DeltaH=-486 kJ`

Balance the following chemical equations: P_(4(s))+6Cl_(2(g))rarr 4PCl_(3(l))

Balance the following chemical equations: P_(4(s))+Cl_(2(g))rarr PCl_(3(l))

How much heat is evolved when 12 gm of CO reacts with N02 according to the following reaction, 4 CO_((g))+ 2NO_(2(g)) rarr 4CO_(2(g)) + N_(2(g)) DeltaH^@ = -1200kJ

Calculate the calorific value of methane if it burns according to the equation CH_4(g) + 2O_2(g) to CO_2(g) + 2H_2O(l) , DeltaH = -890.0 kJ

Red phosphorus reacts with liquid bromine in an exothermic reaction : 2P_((s))+3Br_(2(l))rarr2PBr_(3(g)) Delta_(r)H^(@)=-243kJ . Calculate the enthalpy change when 2.63g of phosphorus with an excess of bromine in this way.