What mass of hydrochloric acid is needed to decompose 50g of limestone?(1)36.5g(2)73g(3)50g(4)100g?

Question

Answer

Answer

Explanation:

When hydrochloric acid reacts with limestone, it forms calcium chloride, carbon dioxide, and water. The balanced chemical equation is:

CaCO3 + 2HCl → CaCl2 + CO2 + H2O

From the equation, we can see that one mole of CaCO3 reacts with two moles of HCl. The molar mass of CaCO3 is 100 g/mol, and the molar mass of HCl is 36.5 g/mol. Using this information, we can calculate the amount of HCl needed to decompose 50 g of CaCO3.

Solution:

We know that one mole of CaCO3 is equal to 100 g and that we have 50 g of CaCO3. Therefore, we have:

50 g CaCO3 × (1 mol CaCO3/100 g CaCO3) = 0.5 mol CaCO3

According to the balanced chemical equation, one mole of CaCO3 requires two moles of HCl. Therefore, we need:

0.5 mol CaCO3 × (2 mol HCl/1 mol CaCO3) = 1 mol HCl

Finally, we can calculate the mass of HCl needed using its molar mass:

1 mol HCl × 36.5 g/mol = 36.5 g HCl

Therefore, the mass of hydrochloric acid needed to decompose 50 g of limestone is 36.5 g.

Answer:

(1) 36.5g

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