H2(g)+ o2(g)-> H20(l)
(delta)Hf(h20(l)=-286 kj/mol
the total volume of hydrogen needed fill the hindenberg was 2.3 x 15^5 m^3. what is the theoretical yield of heat (that which could have been evolved) when the hindenberg exploded, assuming all the hydrogen reacted?
To calculate the theoretical yield of heat released during the explosion of the Hindenburg, we need to consider the balanced chemical equation and the molar enthalpy of formation.
The balanced chemical equation is as follows:
2H₂(g) + O₂(g) → 2H₂O(l)
From the equation, we see that two moles of hydrogen gas (H₂) react with one mole of oxygen gas (O₂) to produce two moles of water (H₂O).
Given that the molar enthalpy of formation (ΔHf) of water (H₂O) is -286 kJ/mol, this means that for every mole of water formed, 286 kJ of heat is released.
To calculate the theoretical yield of heat released, we need to determine the number of moles of water formed by the given volume of hydrogen gas.
First, let's calculate the number of moles of hydrogen gas:
1. Convert the volume of hydrogen gas into liters by multiplying by the conversion factor:
2.3 x 10^5 m³ x (1000 L/1 m³) = 2.3 x 10^8 L
2. Convert the volume of hydrogen gas from liters to moles using the ideal gas law:
PV = nRT (where P is pressure, V is volume, n is moles, R is the ideal gas constant, and T is temperature)
Assuming the pressure and temperature remain constant, we can simplify the equation to:
V = nRT/P
Let's assume T = 298 K and P = 1 atm (standard conditions):
n = (2.3 x 10^8 L) / [(0.0821 L⋅atm⋅K⁻¹⋅mol⁻¹) × (298 K) / (1 atm)]
n ≈ 9.3 x 10^6 moles
Since the balanced equation tells us that 2 moles of hydrogen gas produce 2 moles of water, the number of moles of water formed will also be 9.3 x 10^6 moles.
Now, multiply the number of moles of water by the molar enthalpy of formation to calculate the theoretical yield of heat:
Theoretical yield of heat = (9.3 x 10^6 moles) × (-286 kJ/mol)
Solving this equation will give us the answer to your question.