If a truck's tires are filled to a pressure of 2.38 atm when they are 25.0 degrees Celsius, what would their pressure be, if the temperature of the
tire goes up to 52.78 degrees Celsius after driving on the highway.

P₂ = 2.60 atm

Explanation:

Given data:

Initial pressure = 2.38 atm

Initial temperature = 25.0 °C

Final pressure = ?

Final temperature = 52.78°C

Solution:

Initial temperature = 25.0 °C (25.0+273 = 298 K)

Final temperature = 52.78°C (52.78+273 = 325.78 K)

According to Gay-Lussac Law,

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

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

2.38 atm / 298 K = P₂/325.78 K

P₂ = 2.38 atm × 325.78 K  / 298 K

P₂ = 775.35 atm. K /293 K

P₂ = 2.60 atm

it is the most commonly accepted one

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.