Question

A balloon is filled to a volume of 1.75 L with 3.00 moles of gas at 25

°C. With pressure and temperature held constant, what will be the
volume of the balloon if 0.60 moles of gas are added?

Answer 1

By applying Avogadro's Law, we can deduce that the new volume of the balloon after adding 0.60 moles of gas to the existing 3.00 moles while keeping pressure and temperature constant would be 2.10 L. This is because the volume of a gas is directly proportional to the number of moles of the gas present.

Step-by-step explanation:

The student's question involves the concept of gas laws in chemistry, where the ideal gas law can be applied to find the change in volume of a gas when additional moles of the gas are added to the system, and pressure and temperature remain constant. We can use Avogadro's Law which states that at constant pressure and temperature, the volume of a gas is directly proportional to the number of moles of gas present.

Initially, the balloon contains 3.00 moles of gas at a volume of 1.75 L. With the addition of 0.60 moles, there will be a total of 3.00 + 0.60 = 3.60 moles. If we let V1 and n1 be the initial volume and number of moles, and V2 and n2 be the final volume and number of moles, according to Avogadro's Law (V1/n1 = V2/n2), the new volume (V2) can be calculated as follows:

V2 = (V1 x n2) / n1 = (1.75 L x 3.60 moles) / 3.00 moles = 2.10 L

Therefore, the new volume of the balloon after adding 0.60 moles of gas would be 2.10 L.

Answer 2

The volume of a gas is directly proportional to the number of moles of gas present, provided that the temperature and pressure are held constant. This relationship can be expressed by the ideal gas law equation:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature.

In this problem, the pressure and temperature are held constant, so the volume of the gas is directly proportional to the number of moles of gas. This means that if we multiply the number of moles of gas by a certain factor, the volume will also be multiplied by that same factor.

The balloon is initially filled with 3.00 moles of gas at a volume of 1.75 L. If 0.60 moles of gas are added, the total number of moles of gas in the balloon becomes 3.00 + 0.60 = <<3+0.6=3.6>>3.6 moles.

To find the volume of the balloon after 0.60 moles of gas are added, we can multiply the initial volume of 1.75 L by the ratio of the final number of moles of gas to the initial number of moles of gas:

V = (1.75 L) * (3.6 moles / 3.00 moles) = 1.75 L * 1.20 = <<1.75*1.20=2.10>>2.10 L

Therefore, if 0.60 moles of gas are added to the balloon while the pressure and temperature are held constant, the volume of the balloon will be 2.10 L.