Question

A sealed metal can was left in a storage room. the pressure inside the can was 1.0 atm at a temperature of 27 "C. A fire in the room heated the can to a point at which the pressure reached 2.5 atm and the can exploded. What was the approximate temperature inside the can Just before it exploded?​

Answer 1

477 °C

Step-by-step explanation:

Step 1: Given data

• Initial pressure (P₁): 1.0 atm

• Initial temperature (T₁): 27 °C

• Final pressure (P₂): 2.5 atm

Step 2: Convert 27 °C to Kelvin

We will use the following expression.

K = °C + 273.15 = 27 + 273.15 = 300 K

Step 3: Calculate the final temperature (T₂)

If we assume constant volume (before the can explodes) and ideal behavior, we can calculate the final temperature using Gay-Lussac's law.

T₁/P₁ = T₂/P₂

T₂ = T₁ × P₂/P₁

T₂ = 300 K × 2.5 atm/1.0 atm = 750 K

In Celsius,

°C = K - 273.15 = 750 - 273.15 = 477 °C