20 gram of calcium carbonate is react with 20 gram of HCL how much carbon dioxide is produced during this reaction
Answers
Answer:
Balanced reaction: \mathrm{CaCO}_{3}+2 \mathrm{HCl} \rightarrow \mathrm{CaCl}_{2}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}
From the reaction,
1 mole of calcium carbonate reacts with 2 moles of Hydrogen chloride and produce 1 mole of carbon dioxide.
Let’s calculate the moles of \mathrm{CaCO}_{3}¬:
Molar mass of \mathrm{CaCO}_{3} = 100 g/mol
Given mass of \mathrm{CaCO}_{3}= 20 g
Moles of \mathrm{CaCO}_{3}=\frac{\text { Mass of } \mathrm{CaCo}_{3}}{\text { Molar mass of } \mathrm{CaCo}_{3}}=\frac{20}{100}=0.20\ \mathrm{mol}
0.20 mol of \bold{\mathrm{CaCO}_{3}} reacts with 0.4 mol of HCl
Let’s calculate the moles of HCl:
Molar mass of HCl = 36.45 g/mol
Given mass = 20 ml
Moles of HCl= \frac{\text { Mass of }\mathrm{HCl}}{\text {Molar mass of }\mathrm{HCl}}=\frac{20}{36.45}=0.548\ \mathrm{mol}
Therefore, \mathrm{CaCO}_{3} is limiting reagent.
0.20 mol of \mathrm{CaCO}_{3} gives 0.20 mol of \mathrm{CO}_{2}
Molar mass of \mathrm{CO}_{2} = 44 g/mol
Mass of \mathrm{CO}_{2}\ produced = 0.2 \times 44 \frac{g}{m o l}=8.8 g
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Answer:
Here the moles of CaCO3 = Mass of CaCO3/
Molecular Mass
n= 20/100
n= 0.2
Moles of HCl = 20/36.5 = 0.54 mol
The reaction is
CaCO3 + 2HCl = CaCl2 + CO2 + H2O
For 2 mol of HCl, 1 mol CaCO3 is req.
This means for 0.54 mol HCl, 0.27 mol CaCO3 would be req.
But only 0.2 mol CaCO3 is present.
This means CaCO3 is Limiting Reagent.
For 1 mol CaCO3, 1 mol CO2 is formed.
Therefore moles of CO2 produced = 0.27
Mass of CO2 = 44 × 0.27
= 11.88 gm
Explanation:
Balanced reaction: \mathrm{CaCO}_{3}+2 \mathrm{HCl} \rightarrow \mathrm{CaCl}_{2}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}
From the reaction,
1 mole of calcium carbonate reacts with 2 moles of Hydrogen chloride and produce 1 mole of carbon dioxide.
Let’s calculate the moles of \mathrm{CaCO}_{3}¬:
Molar mass of \mathrm{CaCO}_{3} = 100 g/mol
Given mass of \mathrm{CaCO}_{3}= 20 g
Moles of \mathrm{CaCO}_{3}=\frac{\text { Mass of } \mathrm{CaCo}_{3}}{\text { Molar mass of } \mathrm{CaCo}_{3}}=\frac{20}{100}=0.20\ \mathrm{mol}
0.20 mol of \bold{\mathrm{CaCO}_{3}} reacts with 0.4 mol of HCl
Let’s calculate the moles of HCl:
Molar mass of HCl = 36.45 g/mol
Given mass = 20 ml
Moles of HCl= \frac{\text { Mass of }\mathrm{HCl}}{\text {Molar mass of }\mathrm{HCl}}=\frac{20}{36.45}=0.548\ \mathrm{mol}
Therefore, \mathrm{CaCO}_{3} is limiting reagent.
0.20 mol of \mathrm{CaCO}_{3} gives 0.20 mol of \mathrm{CO}_{2}
Molar mass of \mathrm{CO}_{2} = 44 g/mol
Mass of \mathrm{CO}_{2}\ produced = 0.2 \times 44 \frac{g}{m o l}=8.8 g
Click to let others know, how helpful is it
4.0
137 votes
anasuyab46
anasuyab46Ambitious
Answer:
Here the moles of CaCO3 = Mass of CaCO3/
Molecular Mass
n= 20/100
n= 0.2
Moles of HCl = 20/36.5 = 0.54 mol
The reaction is
CaCO3 + 2HCl = CaCl2 + CO2 + H2O
For 2 mol of HCl, 1 mol CaCO3 is req.
This means for 0.54 mol HCl, 0.27 mol CaCO3 would be req.
But only 0.2 mol CaCO3 is present.
This means CaCO3 is Limiting Reagent.
For 1 mol CaCO3, 1 mol CO2 is formed.
Therefore moles of CO2 produced = 0.27
Mass of CO2 = 44 × 0.27
= 11.88 gm