A balloon at 32 °C is filled with 21 L of air. What would its volume be at a temperature of 52 °C, assuming pressure remains constant?
Assuming the gas is ideal, we use Charles' Law to relate the relationship between Temperature & Volume of gas:
V1/T1 = V2/T2
where:
T1 = initial temperature of gas (in K)
T2 = final temperature of gas (in K)
V1 = initial volume of gas
V2 = final volume of gas
*note that to convert °C to K, we just add 273.
substituting,
(21)/(32 + 273) = V2/(52 + 273)
V2 = (21)*(325)/(305)
V2 = ?
now solve for V2.
hope this helps~ :)
Bruh it's not that hard they literally gave the equation to you it's 22 L. lord save this generation
I wanted the full answer fam fym solve for V2 Bit!!! you solve for it!!
To solve this problem, we can use the ideal gas law formula, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
In this case, we are assuming that the pressure remains constant. So, we can rewrite the formula as V1/T1 = V2/T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume, and T2 is the final temperature.
Now, let's convert the temperatures from Celsius to Kelvin. To do that, we add 273 to each temperature. So, the initial temperature is 32 + 273 = 305 K, and the final temperature is 52 + 273 = 325 K.
We are given that the initial volume is 21 L, and we need to find the final volume.
Using the formula V1/T1 = V2/T2, we can plug in the values: (21 L)/305 K = V2/325 K.
To find V2, we cross-multiply and solve for V2:
(21 L) * 325 K = V2 * 305 K.
V2 = (21 L * 325 K) / 305 K = 22.3 L (rounded to one decimal place).
Therefore, the volume of the balloon at a temperature of 52 °C, assuming constant pressure, would be approximately 22.3 liters.