Question

Calculate to three significant digits the density of chlorine pentafluoride gas at exactly and exactly . You can assume chlorine pentafluoride gas behaves as an ideal gas under these conditions.

Answer 1

Answer:

Density is 6.16g/L

Explanation:

... at exactly -15°C and exactly 1atm...

Using general gas law:

PV = nRT

We can find density (Ratio of mass and volume) in an ideal gas as follows:

P/RT = n/V

To convert moles to grams we need to multiply the moles with Molar Weight, MW:

n*MW = m

n = m/MW

P/RT = m/V*MW

P*MW/RT = m/V

Where P is pressure: 1atm;

MW of chlorine pentafluoride: 130.445g/mol

R is gas constant: 0.082atmL/molK

And T is absolute temperature: -15°C+273.15 = 258.15K

Replacing:

P*MW/RT = m/V

1atm*130.445g/mol / 0.082atmL/molK*258.15K = m/V

6.16g/L = m/V

Density of the gas is 6.16g/L

Answer 2

The density of ClF₅ at exactly -15 °C and exactly 1 atm is 6.16 g/L.

First, we will convert -15 °C to Kelvin using the following expression.

K = °C + 273.15 = -15 °C + 273.15 = 258 K

We want to calculate the density of ClF₅ at exactly 258 K and exactly 1 atm.

What is density?

The density (ρ) of a substance is its mass per unit volume.

For an ideal gas, we can calculate its density using the following expression.

ρ = P × M / R × T

ρ = 1 atm × (130.45 g/mol) / (0.0821 atm.L/mol.K) × 258 K = 6.16 g/L

where

• P is the pressure of the gas.

• M is the molar mass of the gas.

• R is the ideal gas constant.

• T is the absolute temperature.

The density of ClF₅ at exactly -15 °C and exactly 1 atm is 6.16 g/L.

Learn more about ideal gases here: https://brainly.com/question/8711877

Calculate to three significant digits the density of chlorine pentafluoride gas at exactly -15 °C and exactly 1 atm. You can assume chlorine pentafluoride gas behaves as an ideal gas under these conditions.