Question

the gas in a 225.0 ml piston experiences a change in pressure from 1.00 atm to 2.90 atm. what is the new volume (in ml) assuming the moles of gas and temperature are held constant? 7 7 . 5 9

Answer 1

The new volume of a gas, when the pressure is increased from 1.00 atm to 2.90 atm while keeping temperature and moles constant, can be found using Boyle's Law. By applying the formula P1V1 = P2V2 and solving for the new volume V2, the resulting volume is approximately 77.59 ml.

Step-by-step explanation:

The question concerns the relationship between the pressure and volume of a gas, which is described by Boyle's Law. According to Boyle's Law, for a given amount of gas at constant temperature, the pressure of the gas is inversely proportional to its volume. This means that if the pressure increases, the volume decreases proportionally, and vice versa, as long as the temperature and the number of moles of gas remain constant.

Using the formula P1V1 = P2V2, where P represents pressure and V represents volume, we can calculate the new volume after a change in pressure. Initially, the gas has a pressure P1 of 1.00 atm and a volume V1 of 225.0 ml. After the pressure change to P2 of 2.90 atm, we want to find the new volume V2.

The equation becomes:
1.00 atm × 225.0 ml = 2.90 atm × V2
V2 = (1.00 atm × 225.0 ml) / 2.90 atm
V2 = 225.0 ml / 2.90
V2 ≈ 77.59 ml

Therefore, the new volume of the gas when the pressure is increased to 2.90 atm, while keeping the temperature and the moles of gas constant, is approximately 77.59 ml.

Answer 2

Using Boyle's Law, which states that pressure and volume are inversely proportional for a given amount of gas at constant temperature, the new volume of the gas when the pressure is increased from 1.00 atm to 2.90 atm is calculated to be 77.59 mL.

Step-by-step explanation:

The question involves the application of Boyle's Law, which states that for a fixed amount of an ideal gas kept at a constant temperature, the product of the pressure and volume is constant.

The initial conditions are given as a volume (V1) of 225.0 mL and a pressure (P1) of 1.00 atm. The final pressure (P2) is 2.90 atm, and we need to calculate the new volume (V2). Applying Boyle's Law:

P1V1 = P2V2

Now, we solve for V2:

V2 = (P1V1) / P2

Substituting the known values:

V2 = (1.00 atm * 225.0 mL) / 2.90 atm

V2 = 225.0 mL / 2.90

V2 = 77.59 mL

The new volume of the gas, while keeping the moles of gas and temperature constant, is 77.59 mL.