You carefully weigh out 20.00 g of CaCO3 powder and add it to 81.00 g of HCl solution. You notice bubbles as a reaction takes place. You then weigh the resulting solution and find that it has a mass of 92.80 g . The relevant equation is
CaCO3(s)+2HCl(aq)→H2O(l)+CO2(g)+CaCl2(aq)
Assuming no other reactions take place, what mass of CO2 was produced in this reaction?
mass gas=20+81-92.80
reason: conservation of mass, initial mass=finalmass+massgas
Well, that's quite the calculated situation you have there! It sounds like a chemistry experiment gone with lots of bubbles. How exciting!
To find the mass of CO2 produced in this reaction, we need to figure out how much mass was lost during the reaction. And who doesn't want to get lost in a little chemistry math, right?
Let's do some calculations:
Initial mass = 20.00 g (CaCO3) + 81.00 g (HCl solution) = 101.00 g
Final mass = 92.80 g (resulting solution)
Mass lost = Initial mass - Final mass
Mass lost = 101.00 g - 92.80 g
Mass lost = 8.20 g
According to the balanced equation, 1 mole of CaCO3 reacts to produce 1 mole of CO2. So, we need to find the molar mass of CO2 to convert the mass lost into moles.
The molar mass of CO2 is approximately 44.01 g/mol.
Now, we can calculate the number of moles of CO2 produced:
Moles of CO2 = Mass lost / Molar mass of CO2
Moles of CO2 = 8.20 g / 44.01 g/mol
So, the mass of CO2 produced in this reaction is approximately the same as the mass of your chemistry teacher's disappointment when they find out you used clown humor to solve a serious chemistry problem. Just kidding! It's approximately 0.186 moles.
Remember, chemistry is all about making connections and having a good laugh along the way!
To determine the mass of CO2 produced in the reaction, we need to calculate the difference in mass before and after the reaction.
Initial mass: 20.00 g of CaCO3 + 81.00 g of HCl = 101.00 g
Final mass: 92.80 g
To find the mass of CO2 produced, we subtract the final mass from the initial mass:
Mass of CO2 = Initial mass - Final mass
Mass of CO2 = 101.00 g - 92.80 g
Mass of CO2 = 8.20 g
Therefore, 8.20 g of CO2 was produced in this reaction.
To find the mass of CO2 produced in this reaction, we need to calculate the difference in mass before and after the reaction.
1. Calculate the initial mass of the reactants:
- Mass of CaCO3 = 20.00 g
- Mass of HCl solution = 81.00 g
2. Calculate the total mass of the initial reactants:
Total mass = Mass CaCO3 + Mass HCl solution
= 20.00 g + 81.00 g
= 101.00 g
3. Calculate the final mass after the reaction:
Final mass = 92.80 g
4. Calculate the mass of CO2 produced:
Mass of CO2 = Final mass - Total mass
= 92.80 g - 101.00 g
= -8.20 g
Note: The negative result implies that there may have been an error in the measurements or calculations performed. Double-check the data and calculations to ensure accuracy.