You carefully weigh out 17.00g of CaCo3 powder and add it to 68.85g 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 78.88g . 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?

Is mass conserved?

mass reactants = mass products-CO2

15

To find the mass of CO2 produced in this reaction, we need to determine the change in mass before and after the reaction. Here's how you can calculate it step by step:

1. Calculate the initial mass of the reactants:
Mass of CaCO3 = 17.00 g
Mass of HCl solution = 68.85 g

2. Calculate the final mass of the solution after the reaction:
Mass of resulting solution = 78.88 g

3. Find the difference in mass before and after the reaction:
Change in mass = Final mass - Initial mass
= 78.88 g - (17.00 g + 68.85 g)
= 78.88 g - 85.85 g
= -6.97 g

4. Since the change in mass is negative, it means that there was a net mass loss during the reaction.

5. The mass of CO2 produced is equal to the absolute value of the change in mass:
Mass of CO2 produced = |Change in mass|
= |-6.97 g|
= 6.97 g

Therefore, 6.97 grams of CO2 were produced in this reaction.

7.48

7.47