Which statement about the following reaction is correct?

cao (s) + h2o (l) > ca(oh) 2 (s) deltah = -65.2 kj

65.2 kj of heat is absorbed for every one of cao that reacts.
130 kj of heat is released for every mole of h2o that reacts.
32.6 kj of heat is released for every 0.5 mole of cao that reacts.
16.3 kj of heat is absorbed for every 0.5 moles of h2o that reacts.

Since delta H is negative, that means that heat is released, so that eliminates two answers. Since the second response says that twice the delta H value is released for every mole of H2O, that mean that there would have to be a coefficient of 2 in front of H2O for that statement to be true. The next response says that half of the delta H value is released when half of CaO reacts. Since this response is consistent in that if an entire mole of CaO reacts, then the full delta H value would released. So the third response is correct

1. and 2. question: in which equation? or i don't understand you, 3. a), 4. c), 5. c), 6. b), 7. d), 8. d) if small number is underlined(behind symbol) , b) if big number is underlined(in front of symbol)9. what is underlined there? 10. c)