If the values of Delta_(f) H^(@) for H_(2) O_(2) and H_(2) O are -188 and -286 "kJ mol"^(-1), then the value of Delta H^(@) = …. kJ for the following reaction - 2H_(2) O_(2(l)) to 2H_(2)O_((l)) + O_(2(g))

If the values of Delta_(f) H^(@) for H_(2) O_(2) and H_(2) O are -188

1.	If the values of Delta_(f) H^(@) for H_(2) O_(2) and H_(2) O are -188 and -286 "kJ mol"^(-1), then the value of Delta H^(@) = …. kJ for the following reaction - 2H_(2) O_(2(l)) to 2H_(2)O_((l)) + O_(2(g))
Answer» `-494` `-196` `-98` `+196` ANSWER :B