Question

Use the reaction and bond information to answer the question.

H2 + CO2 → CH2O2

Reactant bond energies: H–H is 432 kJ/mol, C=O is 799 kJ/mol

Product bond energies: C–H is 413 kJ/mol, C=O is 745 kJ/mol, C–O is 358 kJ/mol, O–H is 467 kJ/mol

Is this system endothermic or exothermic, and why?

(1 point)

A.) It is endothermic because more energy is needed to break up the reactants versus the amount given off by the products.

B.) It is exothermic because more energy is needed to break up the reactants versus the amount given off by the products.

C.) It is exothermic because more energy is given off by the products versus the amount needed to break up the reactants.

D.) It is endothermic because more energy is given off by the products versus the amount needed to break up the reactants.

Answer 1

Forgot to say what i think it is

Answer 2

I think it’s A

Answer 3

if someone would let me know i would really appreciate it :)

Answer 4

hey are yoi doing CA?

Answer 5

1 Absorbed

2 O=O

3 2,030 kJ

4 Yes, it would occur without additional energy because the reaction is exothermic.

5 The reaction is endothermic, because stronger bonds are broken than formed.

Answer 6

I believe i am, and for anyone wondering A was correct :)