Question

A sealed container of gas is taken out of the refrigerator at 4°C where the pressure is

1 atm. What would the pressure of the container be if it is left outside and is now
48°C?

Answer 1

To find the new pressure of a seal container of gas when left outside at a different temperature, you can use the ideal gas law equation. By plugging in the initial temperature, pressure, and volume, and solving for the new pressure, you can calculate the answer.

Step-by-step explanation:

In this scenario, we can use the ideal gas law to solve for the new pressure of the gas in the sealed container. The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.

First, convert the initial temperature of 4°C to Kelvin by adding 273.15: 4°C + 273.15 = 277.15 K. Then, convert the final temperature of 48°C to Kelvin: 48°C + 273.15 = 321.15 K.

Now we can set up the equation and solve for the new pressure:

P₁V₁/T₁ = P₂V₂/T₂

Plugging in the initial temperature, the initial pressure of 1 atm, and the initial volume of the container, we have:

(1 atm)(V₁)/(277.15 K) = (P₂)(V1)/(321.15 K)

Simplifying the equation, we have:

P₂ = (1 atm)(V₁)(321.15 K)/(277.15 K)

P₂ ≈ 1.16atm