The change in enthalpy of the reaction `2P(s)+3Br_(2)(l)rarr2PBr_(3)(l)" is "-354"`kJ/mol.In this reaction,if the amount of phosphorous consumed is 3.1g ,the change in enthalpy in kJ.[Atomic weight of P = 31] ]

The enthalpy change (Delta H) for the reaction N_(2) (g)+3H_(2)(g) rarr 2NH_(3)(g) is -92.38 kJ at 298 K . What is Delta U at 298 K ?

The enthalpy change (DeltaH) for the reaction, NH_(2(g))+3H_(2(g)) rarr 2NH_(3g) is -92.38kJ at 298K What is DeltaU at 298K ?

Enthalpy change for the reaction, 4H_((g))rarr 2H_(2(g)) is -869.6 kJ The dissociation energy of H-H bond is :

Red phosphorus reacts with liquid bromine in an exothermic reaction 2P(s) + 3 Br_(2) (l) rarr PBr_(3) (g), Delta_(r) H^(@) = - 243 kJ mol^(-1) Calculated the enthalpy change when 2.63 g of phosphorus reacts with an excess of bromine in this way.

Red phosphorus reacts with liquid bromine in an exotermic 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.