PLS HELP! Which of the following statements about the reaction below is true?

3NaHCO3(aq) + C2H3O2(aq) —> 3CO2(g) + 3H2O(l) +NaC2H3O2(aq)

a. 22.4 L of CO2 (g) are produced for every liter of C2H3O2 (aq) reacted.
b. 1 mole of water is produced for every mole of carbon dioxide produced.
c. 6.02 x1023 molecules of NaC2H3O2 (aq) are produced for every mole of NaHCO3(aq) used.
d. 54 g of water are produced for every mole of NaHCO3(aq) produced.

a) false

b) true

c) false

d) false

Explanation:

Step 1: Data given

Molar mass H2O = 18.02 g/mol

Number of Avogadro = 6.022 * 10^23

Step 2: The balanced equation

3NaHCO3(aq) + C2H3O2(aq) —> 3CO2(g) + 3H2O(l) +NaC2H3O2(aq)

a. 22.4 L of CO2 (g) are produced for every liter of C2H3O2 (aq) reacted.

False, for every liter C2H3O2 we'll have 3 liter of CO2

b. 1 mole of water is produced for every mole of carbon dioxide produced.

True, For 3 moles NaHCO3 we need 1 mol C2H3O2 to produce 3 moles CO2, 3 moles H2O and 1 mol NaC2H3O2

c. 6.02 x1023 molecules of NaC2H3O2 (aq) are produced for every mole of NaHCO3(aq) used.

False, for every 3 moles NaHCO3 we'll have 1 mol NaC2H3O2. This means for every mol NaHCO3 we'll have 1/3 * 6.02*10^23 molecules of NaC2H3O2

d. 54 g of water are produced for every mole of NaHCO3(aq) produced.

False, for every mol NaHCO3 we'll have 1 mol H2O produced

1 mol H2O = 18.02 grams of H2O

m=9

step-by-step explanation: