Answer :
Final answer:
Using the ideal gas law and relating initial and final conditions of pressure and temperature, we can find that the final temperature of the helium gas, when its pressure is increased from 210 torr to 1400 torr, is approximately 1861.96 °C.
Explanation:
This physics question pertains to the use of the ideal gas law, a chemistry and physics principle that describes how gases behave. The ideal gas law is expressed as PV = nRT, with P representing pressure, V for volume, n for the number of moles of gas, T for the temperature in Kelvin, and R, the ideal gas constant. Given that we're holding n and V as constants, and as per the direct relationship between pressure and temperature (Gay-Lussac's Law); we can manipulate this law to solve our problem.
First, let's convert temperatures into Kelvin scale, so T1=0+273.15=273.15 K. Next, rearrange the Ideal Gas Law equation to isolate T: T = PV/nR -> T = P/R (as n and V are constant). This allows us to set up a proportion to find the final temperature: (P1/T1) = (P2/T2). Plugging our values into this equation, we have: (210/273.15) = (1400/T2). Solving for T2 gives us a temperature in Kelvin, which we then convert back to Celsius to find that the final temperature is 1861.96 Celsius.
Learn more about Ideal Gas Law here:
https://brainly.com/question/30458409
#SPJ11
