The beakers on the left and right both contain the same amount of HCL (liquid) and the same mass of calcium carbonate (solid). I
n which beaker will the reaction rate be the greatest?
A) The reaction rate will be highest in beaker 1 because there is a larger surface area of calcium carbonate.
B) The reaction rate will be highest in beaker 2 because there is a larger surface area of calcium carbonate.
C) The reaction rate will be highest in beaker 1 because there is a smaller surface area of calcium carbonate.
D) The reaction rate will be highest in beaker 2 because there is a smaller surface area of calcium carbonate
A) The reaction rate will be highest in beaker 1 because there is a larger surface area of calcium carbonate.
B) The reaction rate will be highest in beaker 2 because there is a larger surface area of calcium carbonate.
C) The reaction rate will be highest in beaker 1 because there is a smaller surface area of calcium carbonate.
D) The reaction rate will be highest in beaker 2 because there is a smaller surface area of calcium carbonate
1 answer:
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Answer:
Final temperature of solution is 27.48
Explanation:
Total volume of mixture = (60.0+60.0) mL = 120.0 mL
We know, density = (mass)/(volume)
So mass of mixture =
Amount of heat released per mol of =
Where, m represents mass , C represents specific heat, represents change in temperature and n is number of moles
As this reaction is an exothermic reaction therefore temperature of mixture will be higher than it's initial temperature.
Let's say final temperature of mixture is T
So,
Here and
Moles of H_{3}PO_{4} are added = = 0.012 moles
So,
or, T = 27.48
So, final temperature of solution is 27.48