Suppose 275 g of NO3- flows into a swamp each day. What volume of CO2 would be produced each day at 17.0°C and 1.00 atm? I attached the image of the equation for reference

The volume of produced has been 264.28 L.

The volume of the carbon dioxide gas produced can be calculated with the ideal gas equation.

The moles of has been:

Moles =

Moles of 275 g   has been:

Moles =

Moles of   = 4.44 moles

The balanced equation gives that with the reaction of 2 moles , 5 moles carbon dioxide has been formed.

Moles of carbon dioxide formed with 4.44 mol has been:

2 moles = 5 moles

4.44 moles  = 11.1 moles .

The volume of the can be calculated as:

Pressure Volume = moles Rydberg constant temperature

For the produced:

1 atm Volume = 11.1 mol 0.0821 atm.L/K.mol 290 K

Volume = 264.28 L.

The volume of produced has been 264.28 L.

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264.28 L of CO₂

Explanation:

We'll begin by calculating the number of moles present in 275 g of NO₃¯. This can be obtained as follow:

Mass of NO₃¯ = 275 g

Molar mass of NO₃¯ = 14 + (16×3) = 14 + 48 = 62 g/mol

Mole of NO₃¯ =?

Mole = mass / molar mass

Mole of NO₃¯ = 275 / 62

Mole of NO₃¯ = 4.44 moles

Next, we shall determine the number of mole of CO₂ produced from the reaction. This can be obtained as follow:

2NO₃¯ + 5CO + 2H⁺ —> N₂ + H₂O + 5CO₂

From the balanced equation above,

2 moles of NO₃¯ reacted to produced 5 moles of CO₂.

Therefore, 4.44 moles of NO₃¯ will react to produce = (4.44 × 5) / 2 = 11.1 moles of CO₂.

Thus, 11.1 moles of CO₂ were produced from the reaction.

Finally, we shall determine the volume of CO₂ produced each day. This can be obtained as follow:

Temperature (T) = 17 °C = 17 °C + 273 = 290 K

Pressure (P) = 1 atm

Number of mole (n) of CO₂ = 11.1 moles

Gas constant (R) = 0.0821 atm.L/Kmol

Volume (V) of CO₂ =?

PV = nRT

1 × V = 11.1 × 0.0821 × 290

V = 264.28 L

Thus, 264.28 L of CO₂ would be produced each day.