Answer:
A. yes
594°C
Explanation:
There is some info missing. I think this is the original question.
For many purposes we can treat ammonia (NH₃) as an ideal gas at temperatures above its boiling point of -33 °C. Suppose the pressure on a 6.0 m³ sample of ammonia gas at 16.0°C is tripled. Is it possible to change the temperature of the ammonia at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C.
Given data
V₁ = V₂ = 6.0 m³
T₁ = 16.0°C + 273.15 = 289.2 K
T₂ = ?
P₂ = 3 P₁
Assuming constant volume and ideal gas behavior, we can find the new temperature using the Gay-Lussac's law.
[tex]\frac{P_{1}}{T_{1}} =\frac{P_{2}}{T_{2}} \\T_{2}=\frac{P_{2}.T_{1}}{P_{1}} =\frac{3P_{1}.T_{1}}{P_{1}}=3T_{1}=3 \times 289.2K = 867.6K[/tex]
°C = 867.6K - 273.15 = 594°C
