In the reaction below, how would adding more of reactant A offect the equilibrium of the system? (2 points)

Chemistry

1 answer:

WARRIOR [948]4 years ago

8 0

Answer:

Shift it to the right toward the products,

Explanation:

Adding more reactant will increase the concentration of the reactants, to offset this increased concentration, more products will be formed.

An increase in concentration of a specie favors the direction that uses up that specie and lowers its concentration.
If the concentration of the species on the LHS is increased , the equilibrium will shift to the right to maintain the constancy of the equilibrium constant.

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Below is the word equation for the reaction between sodium hydroxide and hydrochloric acid. Identify the reactant(s) in the reac

Goshia [24]

I a chemical reaction, we have the reactants in the left part,followed by an arrow and then the products.

So, the reactants are the two that are in the left part of the equation:

Sodium hydroxide and Hydrochloric acid

3 0

1 year ago

()

const2013 [10]

Answer:

$\large \boxed{\text{-1276 kJ/mol}}$

Explanation:

You calculate the energy required to break all the bonds in the reactants.

Then you subtract the energy needed to break all the bonds in the products.

CH₃CH₂OH + 3O₂ ⟶ 2CO₂ + 3H₂O

Bonds: 5C-H 1C-C 1C-O 1O-H 3O=O 4C=O 6O-H

D/kJ·mol⁻¹: 413 347 358 467 495 799 467

$\Delta H = \sum{D_{\text{reactants}}} - \sum{D_{\text{products}}}\\\sum{D_{\text{reactants}}} = 5 \times 413 + 1 \times 347 + 1 \times 358 + 1 \times 467 + 3 \times 495 = 3237 + 1485\\=\text{4722 kJ}\\\sum{D_{\text{products}}} = 4 \times 799 + 6 \times 467 =3196 + 2802 = \text{5998 kJ}\\\Delta H = 4722 - 5998= \textbf{-1276 kJ} \\ \text{The overall energy change is $\large \boxed{\textbf{-1276 kJ/mol}}$}.$