a volume of 20. l of O2 os warmed from -30c to 85c what is the new volume if the pressure is kept constant
(V1/T1) = (V2/T2)
T must be in kelvin.
To find the new volume of O2 when the pressure is constant, you can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature, assuming constant pressure.
First, let's convert the temperatures from Celsius to Kelvin since temperature values are commonly expressed in Kelvin.
Given:
Initial volume (V₁) = 20 L
Initial temperature (T₁) = -30 °C = 243 K (converted to Kelvin)
Final temperature (T₂) = 85 °C = 358 K (converted to Kelvin)
Using the formula for Charles's Law:
V₁ / T₁ = V₂ / T₂
Substituting the given values into the equation:
20 L / 243 K = V₂ / 358 K
Rearranging the equation to solve for V₂ (the new volume):
V₂ = (20 L / 243 K) × 358 K
V₂ ≈ 29.3 L
Therefore, the new volume of O2, when the pressure is kept constant, is approximately 29.3 liters.
To determine the new volume of 20 L of O2 when warmed from -30°C to 85°C, assuming constant pressure, you can use Charles's Law. Charles's Law states that the volume of a gas is directly proportional to its temperature if the pressure and the amount of gas are held constant.
It is important to note that temperature must be in kelvin (K) for this equation. To convert Celsius to Kelvin, you simply add 273 to the Celsius temperature.
Step-by-step solution:
1. Convert the starting and ending temperatures from Celsius to Kelvin by adding 273.
Initial temperature = -30°C + 273 = 243 K
Final temperature = 85°C + 273 = 358 K
2. Plug the values into Charles's Law equation:
V1 / T1 = V2 / T2
where V1 is the initial volume, T1 is the initial temperature in Kelvin, V2 is the final volume (unknown), and T2 is the final temperature in Kelvin.
20 L / 243 K = V2 / 358 K
3. Simplify the equation:
20 / 243 = V2 / 358
4. Cross-multiply and solve for V2:
V2 = (20 / 243) * 358
V2 ≈ 29.46 L
Therefore, the new volume of O2, when warmed from -30°C to 85°C at constant pressure, is approximately 29.46 L.