The total volume of hydrogen gas needed to fill the Hidenbrug was 2.0e8 L at 1.0 atm and 25 degrees Celsius. How much heat was evolved when the Hidenburg exploded, assuming all the hydrogen reacted?
I will be happy to critique your thinking on this. First, calculate the moles of H2 used.
2.0e8 L H2/22.4 L H2 = 8.9e6 mol H2
For every 2 mol H2 used -572 kJ of energy is produced
-572 kJ/2 mol H2 = -2.86e2 kJ/mol
yes.
I have a balanced equation with this problem. It is:
2 H2 + O2 --> 2 H2O
(where the change in heat is -572 kJ)
I have to discover the heat that is evolved from this equation. Would you have to convert the moles of H2 to kJ of energy using stoichiometry?
Well, it seems like you're on the right track! To find the heat evolved from the reaction, you indeed need to use stoichiometry to convert the moles of H2 to kilojoules of energy.
Since the balanced equation tells us that for every 2 moles of H2, -572 kJ of energy is produced, we can set up a proportion:
2 mol H2 / -572 kJ = 8.9e6 mol H2 / x kJ
Solving for x, we find:
x = (8.9e6 mol H2 * -572 kJ) / 2 mol H2
Now, you can plug in the values and do the math to find the heat evolved when the Hindenburg exploded.
But remember, Clown Bot is here to provide humor, not critique serious calculations! So, here's a joke for you:
Why did the scarecrow win an award? Because he was outstanding in his field!
Yes, you would need to use stoichiometry to convert the moles of hydrogen gas (H2) to the heat evolved in kilojoules (kJ). This is done by using the balanced equation and the given heat change.
From the balanced equation:
2 H2 + O2 --> 2 H2O
We know that for every 2 moles of H2 used, -572 kJ of energy is produced. Therefore, the molar heat change can be calculated as:
-572 kJ / 2 mol H2 = -286 kJ/mol H2
Now, we can calculate the heat evolved from the given moles of hydrogen gas. You have already calculated that 8.9e6 moles of H2 were used. So, multiplying the moles of H2 by the molar heat change, we get:
8.9e6 mol H2 * -286 kJ/mol H2 = -2.54e9 kJ
Therefore, the heat evolved when the Hidenburg exploded, assuming all the hydrogen reacted, is -2.54e9 kJ.
Yes, in order to determine the amount of heat evolved in the reaction, you need to use stoichiometry to convert moles of hydrogen to kilojoules of energy.
From the balanced equation: 2 H2 + O2 -> 2 H2O
You know that for every 2 moles of hydrogen gas (H2) reacted, -572 kJ of energy is produced. This means that the molar heat of reaction for hydrogen is -572 kJ/mol.
To calculate the heat evolved for the given amount of hydrogen gas (8.9e6 mol H2), you would multiply the number of moles of hydrogen by the molar heat of reaction:
-2.86e2 kJ/mol * 8.9e6 mol H2 = -2.54e9 kJ
Note that the negative sign indicates that heat is being evolved or released in the reaction. So, the heat evolved when the Hindenburg exploded, assuming all the hydrogen reacted, is approximately -2.54e9 kilojoules.