The two balanced equations (1) and (2) are for reactions in which gaseous carbon dioxide is produced from the combustion of (1) solid carbon and (2) gaseous carbon monoxide.

1. C(s) + O2(g) -CO2(g) + 94.0 kcal

2. CO(g) + ½ O2(g) - CO2(g) + 67.6 kcal

On the basis of the information given in equation (1) and assuming no change in temperature or pressure, one can correctly conclude that

the rate of reaction is rapid

the total number of moles of products is the same as the total number of moles of reactants

the reaction is exothermic

the weights of the products are greater

Question

The two balanced equations (1) and (2) are for reactions in which gaseous carbon dioxide is produced from the combustion of (1) solid carbon and (2) gaseous carbon monoxide.

1. C(s) + O2(g) ->CO2(g) + 94.0 kcal

 2. CO(g) + ½ O2(g) -> CO2(g) + 67.6 kcal

On the basis of the information given in equation (1) and assuming no change in temperature or pressure, one can correctly conclude that

the rate of reaction is rapid

the total number of moles of products is the same as the total number of moles of reactants

the reaction is exothermic

the weights of the products are greater

anonymous · Answer

even if you're given heat of enthalpy, you can't conclude anything about the kinematics of the reaction (no way to tell whether rxn is rapid). So first one is not the answer.

Second is also not answer and also is not true. If you look at the first equation, you need a total of 2 mols reactants to make a mole of product.

Third answer is right, since the enthalpy is on the right of the equation. This implies the heat is produced as a product of combustion, which suggests that the rxn is exothermic.

Fourth answer: the wordings is a bit confusing to me. Is it talking about the molecular weight or the mass of the products? If it's talking about the mass of the product, then it can't be greater because it'll violate the law of conservation of mass.

aaronandyson · Answer

The reaction is exothermic.