A chunk of limestone, which is calcium carbonate, reacts with acid. How might you increase the rate of this reaction?
2 answers:
Answer: Option (b) is the correct answer.
Explanation:
When calcium carbonate is added to an acid then the reaction will be as follows.
The formed is easily soluble in water.
Therefore, when we crush calcium carbonate the surface area of particles will increase. As a result more number of molecules will be dispersed in the acid, hence more is the number of calcium carbonate particles more readily the reaction will occur.
Thus, we can conclude that the rate of this reaction increases when we crush the lime stone or calcium carbonate.
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32.8 g of Butane is required and 99.3 g of CO₂ is produced
<u>Explanation:</u>
The above mentioned reaction can be written as,
C₄H₁₀(g) + 13 O₂(g) → 4CO₂(g) + 5 H₂O(g) where ΔH (rxn)= -2658 kJ
It is given that 1.5 × 10³ kJ of energy is produced, the original reaction says that 2658 kJ of heat is produced, which means that less than one mole of butane is used in the reaction.
That is
of butane reacted
Now this moles is converted into mass by multiplying it with its molar mass = 0.564 mol × 58.122 g / mol
= 32.8 g of butane.
Mass of CO₂ produced = 0.564 ×44.01 g /mol × 4 mol
= 99.3 g of CO₂
Thus 32.8 g of Butane is required and 99.3 g of CO₂ is produced