MHB Find the amount of moles of carbon dioxide produced during the reaction

[mathlearn]

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i.If all the calcium carbonate used in set up X was used up for the reaction, what is the amount of moles of carbon dioxide produced during the reaction ? (Ca = 40, C = 12, O = 16)

My progress:

Molar mass of CaCO₃=(40+12+(16*3))gmol^-1=100 gmol^-1

Molar mass of CO₂=12 + 16* 2 gmol^-1=44 gmol^-1

After that what must be done ?

Many Thanks :)

 

[SuperSonic4]

i.If all the calcium carbonate used in set up X was used up for the reaction, what is the amount of moles of carbon dioxide produced during the reaction ? (Ca = 40, C = 12, O = 16)

My progress:

Molar mass of CaCO₃=(40+12+(16*3))gmol^-1=100 gmol^-1

Molar mass of CO₂=12 + 16* 2 gmol^-1=44 gmol^-1

After that what must be done ?

Many Thanks :)

Now you've worked out the molar mass of your substances you can work out the amount of moles of CaCO3 using the equation [math]n = \dfrac{m}{M_r} \text{ or } \text{moles} = \dfrac{\text{mass}}{\text{molar mass}}[/math]

[math]n_{CaCO_3} = \dfrac{5}{100} = \dfrac{1}{20} = 0.05 \text{mol}[/math]Next consider the balanced reaction that is taking place here which is that of a carbonate with acid

[math]CaCO_{3 (s)} + 2HCl_{(aq)} \rightarrow CaCl_{2 (s)} + CO_{2 (g)} + H_2O_{(l)}[/math]

From the equation above we see that one mole of [math]CaCO_3[/math] produces one mole of [math]CO_2[/math] which means you'll have [math]0.05[/math] moles of [math]CO_2[/math] which is the answer to your question.

 

[mathlearn]

View attachment 6150

Thank you very much :) SuperSonic4