When heated, sodium hydrogen carbonate (NaHCO3) decomposes into sodium carbonate, water and carbon dioxide. 2 NaHCO3 → Na2CO3 + H2O + CO2

Use the balanced equation above to calculate the following:

If 5.00 g of NaHCO3 decomposes, calculate the following:

a. How many moles of CO2 are produced?

b. How many molecules is this?

c. what is the mass of the carbon dioxide produced?​

Ibelieve it's celsius. hope this .

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.