what mass of hydrogen must be reachted with excess nitrogen to produce 5000. J of energy based on the reaction: 3H2+N2--> 2NH4+2709J
3H2+N2--> 2NH3+2709J
Molecular mass of H2=2*1.008=2.016
According to the equation:
3*2.016 g H2 => 2709 J
x g H2 => 5000 J
Use proportion.
This is not correct. The answer is 11.2g i just do not know how to do the problem
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To determine the mass of hydrogen required to produce 5000 J of energy based on the given reaction, we need to use the given energy value and the stoichiometry of the reaction.
Let's analyze the given reaction: 3H2 + N2 -> 2NH4 + 2709 J
From the balanced equation, we can see that for every 3 moles of H2, we get 2709 J of energy. Therefore,
3 moles of H2 produce 2709 J of energy
We can now use this ratio to find the moles of H2 required to produce 5000 J of energy:
(5000 J / 2709 J) = (moles of H2 / 3 moles of H2)
Cross-multiplying, we get:
(5000 J * 3 moles of H2) / 2709 J = moles of H2
Calculating this expression gives us:
moles of H2 = 5.524 moles
Since you want to determine the mass of hydrogen, we need to convert moles to grams. The molar mass of hydrogen (H2) is approximately 2 g/mol. Therefore,
mass of H2 = moles of H2 * molar mass of H2
mass of H2 = 5.524 moles * 2 g/mol
mass of H2 = 11.048 g
Therefore, approximately 11.048 grams of hydrogen must react with excess nitrogen to produce 5000 J of energy based on the given reaction.