How many molecules of CO2 will be produced by the decomposition
of 24.9 mol of Ca(HCO3)2 in the following reaction:
Ca(HCO3)2 => CaO(s) + 2CO2(g) + H2O(g).

2.99×10²⁵ molecules of CO₂ are produced

Explanation:

Decomposition reaction is:

Ca(HCO₃)₂ => CaO(s) + 2CO₂(g) + H₂O(g)

Ratio is 1:2. Let's make a rule of three:

1 mol of bicarbonate can produce 2 moles of CO₂

Therefore, 24.9 moles of bicarbonate may produce, 49.8 moles (24.9 .2 )/1

Let's determine the number of molecules

1 mol has 6.02×10²³ molecules

49.8 moles must have (49.8 . 6.02×10²³) / 1 = 2.99×10²⁵ molecules

oh it is true if thats what you are asking

the dependant variable is spilled water

the independent is the heat