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'.
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The question is incomplete, here is the complete question:
Methane gas and chlorine gas react to form hydrogen chloride gas and carbon tetrachloride gas. What volume of hydrogen chloride would be produced by this reaction if 1.1 mL of methane were consumed? Be sure your answer has the correct number of significant digits.
<u>Answer:</u> The volume of hydrogen chloride produced in the reaction will be 4.4 mL
<u>Explanation:</u>
We are given:
Volume of methane gas = 1.1 mL
The chemical equation for the reaction of methane gas and chlorine gas follows:
Moles of methane gas = 1 mole
Moles of hydrogen chloride gas = 4 moles
The relationship of number of moles and volume at constant temperature and pressure was given by Avogadro's law. This law states that volume is directly proportional to number of moles at constant temperature and pressure.
The equation used to calculate number of moles is given by:
where,
are the volume and number of moles of methane gas
are the volume and number of moles of hydrogen chloride
We are given:
Putting values in above equation, we get:
Hence, the volume of hydrogen chloride produced in the reaction will be 4.4 mL