The reaction below is at dynamic equilibrium. mc004-1.jpg Which statement is true for the equilibrium system? The concentration
2 answers:
Answer: The correct statement is :
'The rate of the forward reaction equals the rate of the reverse reaction'.
Explanation:
Dynamic Equilibrium : A chemical reaction is said to be in equilibrium if the concentration of reactant and products become constant. The rate of the reaction going forward is equal to the rate of reaction going backward. Hence, reversible reaction.
Only rates of the backward and forward reaction are equal not the the concentrations.
According to the given reaction:
Rate of the decomposition of ammonia is equal to the rate of formation of ammonia from hydrogen gas and nitrogen gas.
From the given statements the correct statement is:'
The rate of the forward reaction equals the rate of the reverse reaction'.
You might be interested in
Answer:
1.635 M
Explanation:
Given:
10 mL of 20 volumes Hydrogen Peroxide
Here,
20 volumes of Hydrogen Peroxide means that on decomposition of 1 mL of H₂O₂ 20 mL of O₂ is obtained
also,
means 1 dm³ of H₂O₂ solution produces 20 dm³ oxygen
Now,
at 298K and 1 atm
20 dm³ oxygen = moles
or
= 0.817 moles
also,
2H₂O₂ → 2H₂O + O₂
thus,
1 dm³ of solution must contain 2 × moles of O₂ as moles of H₂O₂
thus,
Number of moles of H₂O₂ = 2 × 0.817
or
Number of moles of H₂O₂ = 1.635 moles
Hence,
For 20 volume hydrogen peroxide is 1.635 M