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How many molecules of carbon dioxide are formed when one milligram of hundred percentage pure calcium carbonate is treated with excess hydrochloric acid?
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Calculation of Carbon Dioxide Molecules formed:
Calcium carbonate (CaCO3) reacts with hydrochloric acid (HCl) to form calcium chloride (CaCl2), water (H2O), and carbon dioxide (CO2). The balanced chemical equation for this reaction is:
CaCO3 + 2HCl -> CaCl2 + H2O + CO2
Step 1: Calculate the molar mass of CaCO3
The molar mass of CaCO3 = 40.08 (Ca) + 12.01 (C) + (3 * 16.00) (3 * O) = 100.09 g/mol
Step 2: Calculate the number of moles of CaCO3 in 1 mg
Number of moles = Mass / Molar mass
Number of moles = 0.001 g / 100.09 g/mol = 0.00000999 mol
Step 3: Calculate the number of moles of CO2 formed
From the balanced chemical equation, 1 mol of CaCO3 produces 1 mol of CO2
Therefore, the number of moles of CO2 formed = 0.00000999 mol
Step 4: Calculate the number of molecules of CO2 formed
1 mol of any substance contains Avogadro's number of molecules (6.022 x 10^23)
Number of molecules of CO2 formed = Number of moles * Avogadro's number
Number of molecules of CO2 formed = 0.00000999 mol * 6.022 x 10^23 = 6.02 x 10^19 molecules
Therefore, when 1 milligram of 100% pure calcium carbonate is treated with excess hydrochloric acid, approximately 6.02 x 10^19 molecules of carbon dioxide are formed.
Calcium carbonate (CaCO3) reacts with hydrochloric acid (HCl) to form calcium chloride (CaCl2), water (H2O), and carbon dioxide (CO2). The balanced chemical equation for this reaction is:
CaCO3 + 2HCl -> CaCl2 + H2O + CO2
Step 1: Calculate the molar mass of CaCO3
The molar mass of CaCO3 = 40.08 (Ca) + 12.01 (C) + (3 * 16.00) (3 * O) = 100.09 g/mol
Step 2: Calculate the number of moles of CaCO3 in 1 mg
Number of moles = Mass / Molar mass
Number of moles = 0.001 g / 100.09 g/mol = 0.00000999 mol
Step 3: Calculate the number of moles of CO2 formed
From the balanced chemical equation, 1 mol of CaCO3 produces 1 mol of CO2
Therefore, the number of moles of CO2 formed = 0.00000999 mol
Step 4: Calculate the number of molecules of CO2 formed
1 mol of any substance contains Avogadro's number of molecules (6.022 x 10^23)
Number of molecules of CO2 formed = Number of moles * Avogadro's number
Number of molecules of CO2 formed = 0.00000999 mol * 6.022 x 10^23 = 6.02 x 10^19 molecules
Therefore, when 1 milligram of 100% pure calcium carbonate is treated with excess hydrochloric acid, approximately 6.02 x 10^19 molecules of carbon dioxide are formed.
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How many molecules of carbon dioxide are formed when one milligram of hundred percentage pure calcium carbonate is treated with excess hydrochloric acid?
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How many molecules of carbon dioxide are formed when one milligram of hundred percentage pure calcium carbonate is treated with excess hydrochloric acid? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about How many molecules of carbon dioxide are formed when one milligram of hundred percentage pure calcium carbonate is treated with excess hydrochloric acid? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for How many molecules of carbon dioxide are formed when one milligram of hundred percentage pure calcium carbonate is treated with excess hydrochloric acid?.
How many molecules of carbon dioxide are formed when one milligram of hundred percentage pure calcium carbonate is treated with excess hydrochloric acid? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about How many molecules of carbon dioxide are formed when one milligram of hundred percentage pure calcium carbonate is treated with excess hydrochloric acid? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for How many molecules of carbon dioxide are formed when one milligram of hundred percentage pure calcium carbonate is treated with excess hydrochloric acid?.
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