A gas with a volume of 525 mL at a temperature of -25°C is heated to 175°C. What is the new volume, in milliliters, of the gas if pressure and number of moles

are held constant?

The new volume, in milliliters, of the gas is 948 L

From the question,

We are to determine the new volume of the gas.

From Charles' law which states that the volume of a fixed mass of gas is directly proportional to the temperature (in Kelvin) provided that the pressure remains constant.

That is,

V ∝ T

Then,

V = kT

Therefore, we can write that

Where is the initial volume

is the initial temperature

is the final volume

and is the final temperature

From the given information,

Putting the values into the formula, we get

∴

V₂ ≅ 948 L

Hence, the new volume, in milliliters, of the gas is 948 L

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Volume V2 = 948.13 ml

Explanation:

Given:

Volume V1 = 525 ml

Temperature T1 = -25°C + 273.15

Volume V2 = ?

Temperature T1 = 175°C + 273.15

Computation:

V1 / T1 = V2 / T2

525 / [-25°C + 273.15] = V2 / [175°C + 273.15]

Volume V2 = 948.13 ml

h let me think

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.