Question

For the reaction

4 H $_{2}$ (g) + CO $_{2}$ (g) → CH $_{4}$ (g) + 2 H $_{2}$ O(g) ${\Delta}$ H= -165 kJ

a. Is the reaction endothermic or exothermic?
b. How many kJ of heat are released when 5.0 moles of CO $_{2}$ react with excess H $_{2}$ ?

c. How many kJ of heat are liberated when 12.9 g of H $_{2}$ react with excess CO $_{2}$ ?

(Enter a number not words.)

Answer 1

+ 래1011) CHACS) DHE-165 kJT 4Hr(8) + Corls) a The reaction is exothermic because the Sign t DH is negative heat is released from the reaction (t means CO is the limitin reagont e cause H is prourdled n excess 165 KJ heat released mole Co SX165KT heat released 5 mole Co = 825KJ heat releasd 825 KJ heet released by 5 mole co, So H is the limtine reasent because Co is provided in exces 16 5 kJ heat released H 16 5 CT heat released 165 12.9 1KT haet releaed 12.98 H = 266.06 KJ heat rel eased So 266.06 KT heat leastd by 12.3 3 H,