Chemistry, 11.01.2021 03:40 qveenjordan6456

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

Suppose 275 g of NO3- flows into a swamp each day. What volume of CO2 would be produced each day at

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Answer from: MissDumb1

The volume of $\rm CO_2$ 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 $\rm NO_3^-$ has been:

Moles = $\rm \dfrac{weight}{molecular\;weight}$

Moles of 275 g $\rm NO_3^-$ has been:

Moles = $\rm \dfrac{275}{62}$

Moles of $\rm NO_3^-$ = 4.44 moles

The balanced equation gives that with the reaction of 2 moles $\rm NO_3^-$ , 5 moles carbon dioxide has been formed.

Moles of carbon dioxide formed with 4.44 mol $\rm NO_3^-$ has been:

2 moles $\rm NO_3^-$ = 5 moles $\rm CO_2$

4.44 moles $\rm NO_3^-$ = 11.1 moles $\rm CO_2$ .

The volume of the $\rm CO_2$ can be calculated as:

Pressure $\times$ Volume = moles $\times$ Rydberg constant $\times$ temperature

For the $\rm CO_2$ produced:

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

Volume = 264.28 L.

The volume of $\rm CO_2$ produced has been 264.28 L.

For more information about the volume of gas, refer to the link:

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Answer from: divadebbgirl1

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.

Answer from: Quest

what's the

Answer from: Quest

Ithink it’s 3 as the answer.

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Suppose 275 g of NO3- flows into a swamp each day. What volume of CO2 would be produced each day at...