And the answer is False,it does not have the same number with particles as the one mole of hydrogen.
A wave with a smaller wavelength has more energy than one with a larger wavelength.
Answer:
The answer to your question is Propane
Explanation:
Data
mass of Propane = 3 g
mass of Oxygen = 10 g
limiting reactant = ?
Balanced chemical reaction
C₃H₈ + O₂ ⇒ H₂O + CO₂
Process
1.- Calculate the molar mass of the reactants
C₃H₈ = (12 x 3) + (8 x 1) = 36 + 8 = 44 g
O₂ = 16 x 2 = 32 g
2.- Calculate the theoretical yield C₃H₈ / O₂ = 44/32 = 1.375
3.- Calculate the experimental yield C₃H₈/O₂ = 3/10 = 0.3
4.- Conclusion
The limiting reactant is Propane because the experimental yield was lower than the theoretical yield.
Answer:
25.0 mol O₂ are required in the second reaction
Explanation:
N₂ (g) + 3H₂ (g) → 2NH₃ (g)
4NH₃ (g) + 5O₂ (g) → 4NO (g) + 6 H₂O(l)
Molar ratio in first reaction is 1:2
For every mol of N₂. I make 2 moles of ammonia. If I have 20 moles of N₂, i'm going to get, 40 moles of ammonia.
In the second reaction, molar ratio between products is 4:5.
If I obtained 40 moles of ammonia in first step, let's prepare the rule of three.
4 moles of ammonia react with 5 moles of O₂
40 moles of ammonia react with ( 40.5) /4 = 25moles