You determine the volume of your plastic bag (simulated human stomach) is 1.08 l. how many grams of nahco3 (s) are required to fill this container given a 49.4% co2 recovery, assuming the other contents in the bag take up a negligible volume compared to the gas. the temperature of the room is 24.5 °c and the atmospheric pressure is 753.5 mmhg.

3.636 grams of sodium bicarbonate is required.

Explanation:

Using ideal gas equation:

PV = nRT

where,

P = Pressure of gas = 753.5 mmHg = 0.9914 atm

()

V = Volume of gas = 1.08 L

n = number of moles of gas = ?

R = Gas constant = 0.0821 L.atm/mol.K

T = Temperature of gas = 24.5 °C= 297.65  K

Putting values in above equation, we get:

Percentage recovery of carbon dioxide gas =  49.4%

Actual moles of carbon dioxide formed: 49.4% of 0.0438 mole

According to reaction ,1 mol is obtained from 2 moles of sodium bicarbonate.

Then 0.02164 moles f carbon dioxide will be obtained from:

Mass of 0.04328 moles pf sodium bicarbonate:

0.04328 mol × 84 g/mol = 3.636 g

3.636 grams of sodium bicarbonate is required.

answer by yourhope:

how do models compare to real-world objects?

d. most models represent a real-world object in a simpler way.

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