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? A)

The equation representing the reaction between sodium bicarbonate and hydrochloric acid is as follows:

The substances and combine in a 1:1 ratio. Therefore, we calculate the quantity of sodium bicarbonate and its molar mass to determine the moles formed.

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We also recognize that the stoichiometric proportions are 1:1:1:1:1, which leads to the conclusion that the moles of equal 24.977 moles.

Next, we apply the ideal gas equation , where P denotes pressure, V refers to volume, R is the gas constant, and T represents the temperature in kelvins. We rearrange to solve for V

The final answer should be expressed in liters, , hence

Response: The right choice is (B)

Clarification:

Initially, we need to find the number of moles of .

Next, we will determine the moles of .

The balanced chemical equation is

From this equation, we derive that

Since 1 mole of produces 1 mole of

Thus, 25 moles of yield 25 moles of

Now we need to compute the volume of .

Utilizing the ideal gas law,

Here,

P = pressure of gas = 1.23 atm

V = volume of gas =?

T = temperature of gas =

n = number of moles of gas = 25 moles

R = gas constant = 0.0821 L.atm/mole.K

Substituting in all the known variables into the ideal gas equation results in

Consequently, the volume of carbon dioxide gas generated is