Aballon containing 546cm of air is heated at 10C if the presure is contain wht will be the volume at 20c
To find the volume of the balloon at 20°C, we can use Charles' Law, which states that the volume of a given amount of gas is directly proportional to its temperature in Kelvin, assuming a constant pressure.
First, we need to convert the temperatures from Celsius to Kelvin. To convert Celsius to Kelvin, we add 273 to the Celsius temperature.
Temperature at 10°C = 10 + 273 = 283 K
Temperature at 20°C = 20 + 273 = 293 K
Next, we can set up the equation using Charles' Law:
(V1 / T1) = (V2 / T2)
V1 = Initial volume = 546 cm^3
T1 = Initial temperature = 283 K
T2 = Final temperature = 293 K (since we need to find the volume at 20°C)
Now, substitute the values into the equation:
(546 / 283) = (V2 / 293)
To solve for V2 (volume at 20°C), we cross-multiply and solve for V2:
(546 * 293) / 283 = V2
V2 ≈ 566.92 cm^3
Therefore, the volume of the balloon at 20°C, assuming constant pressure, will be approximately 566.92 cm^3.