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.

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 as : 2P(s) + 3Br_(2)(l) to 2PBr_(3)(g) Delta_(r)H^(@) = - 243 kJ. Calculate the enthalpy change when 10.32 g of phosphorus reacts with an excess of bromine.

For the reaction C_(2)H_(4(g))+3O_(2(g)) rarr 2CO_(2(g))+2H_(2)O_((l)) the difference between enthalpy change and internal energy change is

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] ]

Diborane is a potential rocket fuel which undergoes combustion according to the reaction, B_(2)H_(6) (g) + 3O_(2) (g) rarr B_(2) O_(3) (s) + 3H_(2) O (g) From the following data, calculate the enthalpy change for the combustion of diborane: (i) 2 B (s) + ((3)/(2)) O_(2) (g) rarr B_(2) O_(3) (s) , Delta H = 0 1273 k J//mol (ii) H_(2) (g) + ((1)/(2)) O_(2) (g) rarr H_(2) O (l), Delta H = -286 kJ//mol (iii) H_(2) O (l) rarr H_(2)O (g) Delta H = 44 kJ//mol (iv) 2B (s) + 3H_(2) (G) rarr B_(2) H_(6) (g), Delta H = 36 kJ//mol