A constant volume of oxygen has a pressure of 4.1 atm at 100 °C and 5.0 atm at 185 °C according to Gay-Lussac's law.
What does Gay-Lussac's law state?
At constant volume, the pressure of an ideal gas is proportional to its absolute temperature.
- Step 1: Convert the temperatures to the absolute scale.
We will do so by adding 273.15 to the Celsius temperature.
T₁: 100 °C + 273.15 = 373 K
T₂: 185 °C + 273.15 = 458 K
- Step 2: Calculate the final pressure of the gas.
We will apply Gay-Lussac's law.
P₁/T₁ = P₂/T₂
P₂ = P₁ × T₂/T₁
P₂ = 4.1 atm × 458 K/373 K = 5.0 atm
A constant volume of oxygen has a pressure of 4.1 atm at 100 °C and 5.0 atm at 185 °C according to Gay-Lussac's law.
Learn more about Gay-Lussac's law here:
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