You have a balloon filled with hydrogen gas which keeps it at a constant pressure, regardless of its volume. The initial volume of the gas is 736 mL at 15.0 C. The gas is heated until it's volume is 2.28 L, what is it's final temperature in degrees Celsius

619.2 °C

Explanation:

Given dа ta:

Initial volume of gas = 736 mL

Initial temperature = 15°C

Final volume = 2.28 L

Final temperature = ?

Solution:

First of all we will convert the temperature into kelvin and mL into L.

Initial temperature = 15°C (15+273 = 288 k)

Initial volume of gas = 736 mL * 1 L/1000 mL = 0.736 L

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

0.736 L / 288 k = 2.28 L / T₂

T₂ = 2.28 L * 288 k/0.736 L

T₂ = 656.64 K / 0.736

T₂ = 892.2 K

Kelvin to °C:

892.2 K - 273.15 = 619.2 °C