What happened to the number of moles in a sample that originally occupied 500mL with 2.50 moles and then occupied 750mL?

2 answers:

7 0

Either you have added an extra half of the # of moles or you changed the condition (lower the pressure or increase the temp.)

ANEK [815]3 years ago

3 0

Answer: The number of moles that initially occupied a 250ml container remains the same when it occupied 750ml container but they are freer because the 750ml container is bigger and has more space. So the gases now occupied more space and their movement is less curtailed unlike when they were in 250ml container

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Question 2 of 50

wolverine [178]

The thermal decomposition of calcium carbonate will produce 14 g of calcium oxide. The stoichiometric ratio of calcium carbonate to calcium oxide is 1:1, therefore the number of moles of calcium carbonate decomposed is equal to the number of moles of calcium oxide formed.

Further Explanation:

To solve this problem, follow the steps below:

Write the balanced chemical equation for the given reaction.
Convert the mass of calcium carbonate into moles.
Determine the number of moles of calcium oxide formed by using the stoichiometric ratio for calcium oxide and calcium carbonate based on the coefficient of the chemical equation.
Convert the number of moles of calcium oxide into mass.

Solving the given problem using the steps above:

STEP 1: The balanced chemical equation for the given reaction is:

$CaCO_{3} \rightarrow \ CaO \ + \ CO_{2}$