2. Suppose you are running a trial of the reaction in Part A. You use 2.80 g of

Question

2. Suppose you are running a trial of the reaction in Part A. You use 2.80 g of NaHCO3, and determine that 2.83 g of carbon dioxide are produced. Using these data and a periodic table, show calculations to:

a. Convert the mass of NaHCO3 to moles using the molar mass of NaHCO3.





b. Convert the mass of CO2 to moles using the molar mass of CO2.





c. Find the simplest ratio between the number of moles of NaHCO3 and CO2. (Hint: Divide both numbers by the smaller of the two to get a ratio.)




The mole ratio of NaHCO3:CO2 is ____:____.


d. Compare this ratio to the ratio of the coefficients for NaHCO3 and CO2 in the three balanced chemical equations (given on page 1). Which of the three possible reactions discussed is consistent with these results? WRITE THE EQUATION HERE.

Explanation / Answer

(a)

Moles of NaHCO3 = mass / molar mass = 2.80 / 84 = 0.0333 mol

(b)

Moles of CO2 = 2.83 / 44 = 0.0643 mol

(c) Simplest ratio, NaHCO3 : CO2

0.0333 / 0.0333   :    0.0643 / 0.0333

1 : 2

(d)

Based on the three equations provided and the result that obtained in (c), you can find the best equation.

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