Answer:

According to the Ideal Gas Law, PV = nRT, where:

- P is the pressure of the gas

- V is the volume of the gas

- n is the number of moles of gas

- R is the universal gas constant (= 0.08206 L•atm/mol•K)

- T is the temperature of the gas in kelvins (K)

At STP (Standard Temperature and Pressure), the temperature is 273.15 K and the pressure is 1 atm.

We can use the ratio of the volumes of the gas at the two different conditions, assuming the number of moles of gas does not change:

(Volume at STP) / (Volume at 35.0°C and 725.0 mmHg) = (Pressure at 35.0°C and 725.0 mmHg) / (Pressure at STP)

Let's solve for (Volume at STP):

(Volume at STP) = (Volume at 35.0°C and 725.0 mmHg) * (Pressure at STP) / (Pressure at 35.0°C and 725.0 mmHg)

We are given that the volume at 35.0°C and 725.0 mmHg is 3.00 L.

Let's convert the pressure values to atmospheres (atm) for consistency:

Pressure at 35.0°C and 725.0 mmHg = 725.0 mmHg * (1 atm / 760.0 mmHg) = 0.9539 atm

(Pressure at STP) = 1 atm

Substituting these values, we get:

(Volume at STP) = (3.00 L) * (1 atm) / (0.9539 atm)

(Volume at STP) = 3.145 L

Therefore, the volume of the gas at STP is approximately 3.145 L.

Explanation:

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