Asample of an ideal gas occupies 2.78 x 10^3 ml at 25°c and 760 mm hg.
what volume will it occupy at the same temperature and 475 mm hg?

The volume that it will occupy at the same temperature is 4448mL

According to Boyle's law, the pressure of a given mass of gas is inversely proportional to the volume. It is expressed mathematically as:

This can be expressed as

Given the following parameters

P₁ = 760mmHg

V₁ = 2.78 x 10³ mL

P₂ = 475mmHg

V₂ = ?

Substitute the given parameters into the formula

Hence the volume that it will occupy at the same temperature is 4448mL

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It will occupy at the same temperature and 475 mm Hg.

Explanation:

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

    (At constant temperature and number of moles)

   (At constant temperature and number of moles)

where,

= initial pressure of gas = 760 mm Hg

= final pressure of gas = 475 mm Hg

= initial volume of gas =

 = final volume of gas = ?

Putting in the values:

Thus it will occupy at the same temperature and 475 mm Hg

answer: i have one answer

acids are substances that ionize (break off) in an aqueous solution to produce hydrogen (h+) ions

explanation:

hope this and sorry i could only come up with one answer!