Question

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 its volume is 2.28 L, what is its final
temperature in degrees Celsius?

Answer 1

619

Step-by-step explanation:

it takes of the 0.2 on CK12

Answer 2

619.2 K

Step-by-step explanation:

We can solve this problem by using Charle's Law, which states that:

"For a fixed mass of an ideal gas kept at constant pressure, the volume of the gas is directly proportional to its absolute temperature"

Mathematically:

`V\propto T`

where

V is the volume of the gas

T is the absolute temperature

The equation can be rewritten as follows for a gas that undergoes a transformation at constant pressure:

`(V_1)/(T_1)=(V_2)/(T_2)`

where in this problem:

`V_1=736 mL = 0.736 L` is the initial volume of the gas

`T_1=15.0C+273=288 K` is the initial temperature

`V_2=2.28 L` is the final volume of the gas

Solving for T2, we find the final temperature:

`T_2=(V_2 T_1)/(V_1)=((2.28)(288))/(0.736)=892.2 K`

Converting into Celsius degrees,

`T_2=892.2-273=619.2 K`