[" 87.The "E^(@)" at "25^(@)C" for the following reaction is "0.55V" .Calculate the "Delta G^(@)" in "kJ/mol" : "," ? "],[qquad 4BiO^(+)(aq)+3N_(2)H_(5)^(+)longrightarrow4Bi(s)+3N_(2)(g)+4H_(2)O(D)+7H^(+)quad 1 gamma']

The E^(@) at 25^(@) C for the following reaction is 0.55 V. Calculate the DeltaG^(@) in kJ // mol : 4BiO^(+)(aq)+3N_(2)H_(5)^(+)to4Bi(s)+3N_(2)(g)+4H_(2)O(l)+7H^(+)

The E^(@) at 25^(@) C for the following reaction is 0.55 V. Calculate the DeltaG^(@) in kJ // mol : 4BiO^(+)(aq)+3N_(2)H_(5)^(+)to4Bi(s)+3N_(2)(g)+4H_(2)O(l)+7H^(+)

The E^(@) at 25^(@) C for the following reaction is 0.55 V. Calculate the DeltaG^(@) in kJ // mol : 4BiO^(+)(aq)+3N_(2)H_(5)^(+)to4Bi(s)+3N_(2)(g)+4H_(2)O(l)+7H^(+)

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

Which is the heat of reaction for the following reaction: CH_(4)(g) + NH_(3)(g) rarr 3H_(2)(g) +HCN(g) Use the following thermodynamic data in kJ/mol. N_(2)(g) + 3H_(2)(g) rarr 2NH_(3) (g) , Delta_(r )H^@ = -91.8 C(s) + 2H_(2)(g) rarr CH_(4)(g), Delta_(r )H^(@) = +74.9 H_(2)(g) + 2C(s) + N_(2)(g) rarr 2HCN(g), Delta_(r )H^(@) = 261.0

Which is the heat of reaction for the following reaction: CH_(4)(g) + NH_(3)(g) rarr 3H_(2)(g) +HCN(g) Use the following thermodynamic data in kJ/mol. N_(2)(g) + 3H_(2)(g) rarr 2NH_(3) (g) , Delta_(r )H^@ = -91.8 C(s) + 2H_(2)(g) rarr CH_(4)(g), Delta_(r )H^(@) = +74.9 H_(2)(g) + 2C(s) + N_(2)(g) rarr 2HCN(g), Delta_(r )H^(@) = 261.0