Given C_("graphite") + O_(2 ) (g) to CO_(2)(g) , Delta _(r) H^(@) = -393.5 kJ mol^(-1) H_(2) (g) + (1)/(2) O_(2) (g) to H_(2) O (l) , Delta_(r) H^(@) = -285.8 kJ mol^(-1) CO_(2) (g)+ 2 H_(2) O (l) to CH_(4) (g) + 2 O_(2) (g) , Delta_(r) H^(@)= + 890 . 3 k J mol^(-1) Based on the above thermochemical equations, the value of Delta_(r)H^(@)at 298 K for the reaction C_("(graphite)") + 2 H_(2) (g) to CH_(4) (g) will be :

Given C_("graphite") + O_(2 ) (g) to CO_(2)(g) , Delta _(r) H^(@) = -

1.	Given C_("graphite") + O_(2 ) (g) to CO_(2)(g) , Delta _(r) H^(@) = -393.5 kJ mol^(-1) H_(2) (g) + (1)/(2) O_(2) (g) to H_(2) O (l) , Delta_(r) H^(@) = -285.8 kJ mol^(-1) CO_(2) (g)+ 2 H_(2) O (l) to CH_(4) (g) + 2 O_(2) (g) , Delta_(r) H^(@)= + 890 . 3 k J mol^(-1) Based on the above thermochemical equations, the value of Delta_(r)H^(@)at 298 K for the reaction C_("(graphite)") + 2 H_(2) (g) to CH_(4) (g) will be :
Answer» `+ 144.0 KJ MOL^(-1)` `-74.8 kJ mol^(-1)` `-144.0 kJ mol^(-1)` `+ 74.0 kJ mol^(-1)` ANSWER :B