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.

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

c. 75.7

i think that is the right

the ratio of the conjugate base to the acid required to attain the desired ph.