Question #0c095

1 Answer
Jun 24, 2017

Answer:

#704^"o""C"#

Explanation:

To solve this, we'll use the temperature-volume relationship of gases, illustrated by Charles's law:

#(V_1)/(T_1) = (V_2)/(T_2)# (constant pressure and quantity)

Remember, when using any gas equation, the value for temperature must always be in Kelvin, so let's convert the temperature to Kelvin

#"K" = 20^"o""C" + 273 = 293# #"K"#

The original volume (#V_1#) is given as #1.50# #"L"#, and the final volume (#V_2#) is #5.00# #"L"#.

Plugging in the values into the equation, and solving for the final temperature (#T_2#), we have

#T_2 = (V_2T_1)/(V_1) = ((5.00cancel("L"))(293color(white)(l)"K"))/(1.50cancel("L")) = color(red)(977# #color(red)("K"#

Which, in Celsius temperature is

#""^"o""C" = 977color(white)(l)"K" - 273 = color(red)(704^"o""C"#