Question 1044097
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The pressure of an ideal gas was held constant. The initial temperature and volume were 600 K and 500 ml respectively. 
What would the final temperature be if the volume were increased to 1500 ml?
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<pre>
Apply the "Ideal gas Law".

See <A HREF=https://en.wikipedia.org/wiki/Ideal_gas_law>this</A> Wikipedia article

   The ideal gas law is the equation of state of a hypothetical ideal gas. 
   It is a good approximation of the behavior of many gases under many conditions, although it has several limitations. 
   It was first stated by Émile Clapeyron in 1834 as a combination of the empirical Boyle's law, Charles' law and Avogadro's Law.
   The ideal gas law is often written as:

   {{{PV}}} = {{{nRT}}}

   where:

   P is the pressure of the gas,
   V is the volume of the gas,
   n is the amount of substance of gas (in moles),
   R is the ideal, or universal, gas constant, equal to the product of the Boltzmann constant and the Avogadro constant,
   T is the absolute temperature of the gas.

For two states of your gas

{{{PV[1]}}} = {{{nRT[1]}}}   and 

{{{PV[2]}}} = {{{nRT[2]}}}.

Now divide left sides and right sides. You will get

{{{V[1]/V[2]}}} = {{{T[1]/T[2]}}}.

Hence, {{{T[2]}}} = {{{T[1]*(V[1]/V[2])}}} = {{{600*(500/1500)}}} = 200 K.
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