Consider the following chemical equations to answer the question that follows. caco3(s)ca(oh)2(s)ca(oh)2(s)+2hcl(g )→cao(s)+co2(g)→h2o(l)+cao(s)→cacl2 (s)+2h2o(l)δhδhδh=175kj=67kj=−198kj using the information above, determine the change in enthalpy for the following chemical reaction. caco3(s)+2hcl(g)⟶cacl2(s)+h2o(l)+co 2(g)

Answer : The change in enthalpy for the following chemical reaction is, -90 kJ

Explanation :

According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.

The given main reaction is,

The intermediate balanced chemical reaction will be,

(1)    

(2)    

(3)    

Now we will reverse the reaction 2 and then adding all the equations, we get :

(1)    

(2)    

(3)    

The expression for enthalpy of change will be,

Therefore, the change in enthalpy for the following chemical reaction is, -90 kJ

a basic solution is an aqueous solution containing more oh-ions than h+ions. in other words, it is an aqueous solution with a ph greater than 7. basic solutions contain ions, conduct electricity, turn red litmus paper blue, and feel slippery to the touch.

explanation:

d.) the average kinetic energy of the gas particles is greater in container b because its particles move faster.