The volume of a gas is 250 mL at 340.0 kPa pressure. What will the volume be when the pressure is reduced to 50.0 kPa, assuming the temperature remains constant?
P1V1 = P2V2
88.7mL of ammonia, NH3.
To solve this problem, we can use Boyle's Law, which states that the volume of a gas is inversely proportional to its pressure, assuming the temperature remains constant.
Mathematically, Boyle's Law can be expressed as:
P₁V₁ = P₂V₂
where:
P₁ = initial pressure (in kPa)
V₁ = initial volume (in mL)
P₂ = final pressure (in kPa)
V₂ = final volume (unknown)
Given data:
P₁ = 340.0 kPa
V₁ = 250 mL
P₂ = 50.0 kPa
Substituting the given values into the equation, we get:
340.0 kPa * 250 mL = 50.0 kPa * V₂
Now, we can solve for V₂ by rearranging the equation:
V₂ = (340.0 kPa * 250 mL) / 50.0 kPa
V₂ = 1700 mL
Therefore, the volume of the gas will be 1700 mL when the pressure is reduced to 50.0 kPa, assuming the temperature remains constant.
To solve this problem, we can use Boyle's Law, which states that the volume of a gas is inversely proportional to its pressure, assuming the temperature remains constant. Boyle's Law can be written as:
P1 * V1 = P2 * V2
Where:
P1 and P2 are the initial and final pressures, respectively,
V1 and V2 are the initial and final volumes, respectively.
In this case, we are given:
P1 = 340.0 kPa
V1 = 250 mL
P2 = 50.0 kPa
V2 = ?
To find V2, we will rearrange the equation as follows:
V2 = (P1 * V1) / P2
Now, let's plug in the given values:
V2 = (340.0 kPa * 250 mL) / 50.0 kPa
To make the units consistent, we need to convert milliliters (mL) to liters (L). Since 1 L = 1000 mL, we have:
V2 = (340.0 kPa * 0.250 L) / 50.0 kPa
V2 = 1.700 L
Therefore, the volume of the gas when the pressure is reduced to 50.0 kPa will be 1.700 liters.