Ahot air balloon is filled with 1.35 × 106 l of an ideal gas on a cool morning (11 °c). the air is heated to 127 °c. what is the volume of the air in the balloon after it is heated? assume that none of the gas escapes from the balloon.

Volume = 1.901 * 10^6 liters

Explanation:
We will assume that the pressure of the gas is kept constant.
Charles's law states that: "At constant pressure, the volume of a given mass of gas is directly related to its temperature in kelvin."
This means that:
V1 / T1 = V2 / T2
where:
V1 is the initial volume = 1.35 × 10^6 liters
T1 is the initial temperature = 11 + 273 = 284 degrees kelvin
V2 is the final volume that we want to find
T2 is the final temperature = 127 + 273 = 400 degrees kelvin

Substitute with the givens in the above equation to get the final volume as follows:
V1 / T1 = V2 / T2
(1.35 × 10^6) / (284) = V2 / (400)
V2 = 400 * [(1.35 × 10^6) / (284)]
V2 = 1.901 * 10^6 liters

Hope this helps :)

Answer:

a. energy is absorbed in the reaction.

explanation:

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.