Answer:
0.3192 M
Explanation:
From the question given above, the following data were obtained:
Volume of stock solution (V1) = 5.32 mL Molarity of stock solution (M1) = 6 M
Volume of diluted solution (V2) = 100 mL
Molarity of diluted solution (M2) =?
We can obtain the molarity of the diluted solution by using the dilution formula as shown follow:
M1V1 = M2V2
6 × 5.32 = M2 ×100
31.92 = M2 × 100
Divide both side by 100
M2 = 31.92 / 100
M2 = 0.3192 M
Therefore, the molarity of the diluted solution is 0.3192 M.
Answer:
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Explanation:
The solution is 45.7 % (NH₄)₂CO₃ by mass.
Mass of solution = 0.0332 kg + 0.0395 kg = 0.0727 kg
% (NH₄)₂CO₃ = Mass of (NH₄)₂CO₃/Total mass × 100 % = 0.0332 kg/0.0727 kg × 100 % = 45.7 %
Answer is: reaction is second order with respect to a.
This second order reaction<span> is proportional to the square of the concentration of reactant a.
</span>rate of reaction = k[a]².
k is second order rate constant and have unit M⁻¹·s⁻¹.
Integrated rate law for this reaction: <span><span>1/[a]</span>=<span>1/<span>[a]</span></span></span>₀ <span>+ kt.
t is time in seconds..</span>