Answer:
I would go for number 5 . It sounds more logical to me.
Answer:
Oxygen
Explanation:
Any Hydrocarbon + Oxygen ----> Carbon Dioxide + H2O (Water vapour, gas, water)
Answer:
10%
Explanation:
Given data:
Actual yield = 0.13 moles
Percent yield = ?
Solution:
Balanced chemical equation.
3H₂ + N₂ → 2NH₃
First of all we will calculate the mass of given moles of ammonia.
Number of moles = mass / molar mass
Mass = 0.13 × 17 g/mol
Mass = 2.21 g
2.21 g is experimental yield of ammonia.
Hydrogen is limiting reactant because only two moles of hydrogen present.
we will compare the moles of hydrogen and ammonia from balance chemical equation.
H₂ : NH₃
3 : 2
2 : 2/3×2 = 1.33 moles
Mass of ammonia
Mass = number of moles × molar mass
Mass = 1.33 mol × 17 g/mol
Mass = 22.61 g
Percent yield:
Percent yield = actual yield / theoretical yield × 100
Percent yield = 2.21 g / 22.61 g
Percent yield =9.8% which is almost 10%
<span>The activation energy was reached was 10:45 a.m. The additional energy did not affect the reaction.</span>
Well, it is a h<span>eterogeneous mixture.... but im not sure EXACTLY what you mix to get the best flavor of ice cream in the world; mint chocolate chip...</span>
