How much CO₂ (L)is produced when 2.10 kg of sodium bicarbonate reacts with excess hydrochloric acid at 25.0 °C and 1.23 atm?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction between sodium bicarbonate and hydrochloric acid is:

NaHCO3 + HCl -> NaCl + CO2 + H2O

From the balanced equation, we can see that for every 1 mole of NaHCO3, we get 1 mole of CO2.

First, we need to convert the mass of NaHCO3 to moles:

2.10 kg NaHCO3 x (1 mol NaHCO3/84.0066 g NaHCO3) = 24.9951 moles NaHCO3

Since sodium bicarbonate is in excess, all of the hydrochloric acid will react with it. We can use the ideal gas law to calculate the volume of CO2 produced:

PV = nRT

V = nRT/P

where P = 1.23 atm, T = 25 + 273 = 298 K, R = 0.08206 L*atm/(mol*K), and n = 24.9951 mol (from above)

V = (24.9951 mol)(0.08206 L*atm/(mol*K))(298 K)/(1.23 atm) = 480.61 L

This is the volume of CO2 at STP (0 °C and 1 atm). To convert to the given conditions (25.0 °C and 1.23 atm), we can use the combined gas law:

P1V1/T1 = P2V2/T2

V2 = V1(P2T1)/(P1T2)

V2 = (480.61 L)(1.23 atm)(298 K)/(1 atm)(298.15 K) = 594.71 L

Finally, we can convert this volume of CO2 at the given conditions to moles using the ideal gas law:

PV = nRT

n = PV/RT

n = (1.23 atm)(594.71 L)/(0.08206 L*atm/(mol*K))(298 K) = 24.9971 moles

Since 1 mole of NaHCO3 produces 1 mole of CO2, the amount of CO2 produced is also 24.9971 moles. We can convert this to mass using the molar mass of CO2:

24.9971 moles CO2 x 44.01 g/mol = 1100.02 g = 4.98 x 10^12 (scientific notation) or 4.98 × 10¹² (standard notation)

Therefore, the answer is B: 4.98 × 10¹².

How Much CO2 (L)is Produced When 2

How Much CO₂ (L)is Produced When 2