00:01
Here we have a question about the explosion of the hindenburg balloon.
00:05
We want to know how much heat evolved during this reaction.
00:09
So the balloon was full of hydrogen gas, which when combusted, reacts with oxygen gas to form water vapor.
00:21
To balance this chemical equation, we need to add a two in front of the water and a two in front of the hydrogen.
00:29
So we know that the total volume of hydrogen gas in the hindenburg was 2 .0 times 10 to the 8 liters.
00:35
At a pressure of one atmosphere and a temperature of 25 degrees celsius.
00:50
We want to know how much heat was evolved, given that the heat of formation, the standard heat of formation for water in this chemical equation, is negative 286 kilojoules per mole.
01:10
So first we need to find the moles of hydrogen gas inside of the hindenburg, convert that into moles of water, and then determine the heat released using this standard heat of formation.
01:23
To do that, we will use our ideal gas law.
01:26
Pressure times volume is equal to moles of gas times the ideal gas constant times temperature, where r is equal to 0 .0821 liters times atmospheres divided by moles times kelvin...
