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An illustration depicting the chemical reaction process between limestone and hydrogen chloride. Start with an image of a pile of limestone represented by its chemical formula, CaCO3, sitting on a scale displaying 25g. Nearby jars labeled with the formulas 'HCl' and 'CaCl2' to represent hydrogen chloride and calcium chloride respectively. Show the reaction sequence with arrows, but do not include any text or numerical values in the image.

Calculate the number of moles of calcium chloride Cacl2 that can be obtained from 25g of limestone CaCo3 in the presence of excess hydrogen chloride

0.25 moles of cacl2 as:

CaCo3+ HCl = CaCl2 + H2CO3
SO 1 mol of CaCO3 will give 1 mol of CaCl2.
mass of CaCO3= 25g
Molar mass of CaCO3= 100g
therefore moles of CaCO3 = 25/100 =0.25
thus 0.25 moles of CaCl2 will be produced

same as moles of CaCO3

CaCO3 = 100 g/mol = 40 + 12 + 48
so we have 0.25 mols of lime and will get 0.25 mols of CaCl2

Calculate the number of moles of calcium chloride (Cacl2) that can be obtained from 25g of limestone (Caco3) in the presence of excess hydrogen chloride (HCl)

Calculate the number of moles of calcium chloride CaCl2 that can be obtained from the 20g linestone CaC3 in the presence of excess hydrogen chloride (Can=40,it=1,C=12 O = 16 ,Cl=35.5)

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Mass of caco3

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Calculate the number of mole of calium chride cacl2 that can be obtaibed from 25g of lime stone. Caco3 in the present of excess of hydrogen chloride hcl (ca 40, (12,o 16, h 1 cl (355)