To determine the resulting pressure when the light bulb containing argon is heated from 18°C to 85°C at constant volume, we can make use of the ideal gas law. The ideal gas law states:
PV = nRT
Where: P = pressure V = volume n = number of moles of gas R = ideal gas constant T = temperature in Kelvin
First, let's convert the given temperatures to Kelvin: Initial temperature (T1) = 18°C + 273.15 = 291.15 K Final temperature (T2) = 85°C + 273.15 = 358.15 K
The volume (V) is stated to be constant, which means it remains the same throughout the process.
Now, let's assume that the number of moles of argon gas (n) remains constant as well. In this case, we can write:
P1V = nRT1 (Initial state) P2V = nRT2 (Final state)
Since V, n, and R are constant, we can set these equations equal to each other:
P1/T1 = P2/T2
Now we can solve for P2, which is the pressure at the final temperature:
P2 = P1 * (T2 / T1) = (1/20) * (358.15 K / 291.15 K) ≈ 0.0912 ATM
Therefore, the resulting pressure when the light bulb is heated to 85°C at constant volume would be approximately 0.0912 ATM.
As for whether this pressure is enough to cause sudden breakage of the bulb, it would depend on the specific properties and strength of the bulb material. Different materials have different thresholds for pressure tolerance. If the pressure exceeds the strength of the bulb, it could potentially cause breakage. It is advisable to consult the manufacturer's specifications or relevant safety guidelines to determine the maximum pressure the bulb can withstand.