Answer:
621.3°C
Step-by-step explanation:
To find the new temperature of the neon gas after it expands from 15.0 liters to 45.0 liters, you can use the Ideal Gas Law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. If the pressure is constant, then P remains constant, so the relationship between volume and temperature can be expressed as:
V1/T1 = V2/T2
where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.
Substituting the initial values:
V1 = 15.0 liters
T1 = 25.0°C + 273.15 = 298.15 K
And the final values:
V2 = 45.0 liters
We can solve for T2:
T2 = T1 * (V2/V1) = 298.15 K * (45.0 liters / 15.0 liters) = 894.5 K
Finally, we can convert T2 back to Celsius:
T2 = 894.5 K - 273.15 = 621.3°C
In conclusion, if 15.0 liters of neon at 25.0°C is allowed to expand to 45.0 liters, the new temperature must be 621.3°C in order to maintain constant pressure.