Answer:
Nitrogen is limiting reactant while hydrogen is in excess.
Explanation:
Given data:
Mass of N₂ = 25 g
Mass of H₂ = 25 g
Mass of ammonia formed = ?
Solution:
Chemical equation:
N₂ + 3H₂ → 2NH₃
Number of moles of Nitrogen:
Number of moles = mass/ molar mass
Number of moles = 25 g/ 28 g/mol
Number of moles = 0.89 mol
Number of moles of hydrogen:
Number of moles = mass/ molar mass
Number of moles = 25 g/ 2 g/mol
Number of moles = 12.5 mol
Now we will compare the moles of both reactant with ammonia.
H₂ ; NH₃
3 : 2
12.5 : 2/3×12.5 = 8.3
N₂ ; NH₃
1 : 2
0.89 : 2×0.89 = 1.78
The number of moles of ammonia produced by nitrogen are less thus nitrogen is limiting reactant while hydrogen is in excess.
Answer:
The balanced equation for methanol when is burned in the air, is
CH3OH + O2 -----> 3/2 CO2 +2 H2O and as you see coefficient of oxygen is 3/2
Explanation:
When you always burn something you are doing combustion. The reactives are your compound + O2, and as products you have CO2 and H2O
Answer: a: extended or controlled release
Explanation:
Electric force is given by:
F = (kQ₁Q₂)/r²
where k is Coloumb's constant of value 9 x 10⁹, Q₁ and Q₂ are charges and r is the separation between them.
Let the charge of the nucleus be located at its center.
The separation of the proton is equal to:
Radius of nucleus + distance from surface
= 3 + 1.8
= 4.8 fm
Charge of Nucleus = 54e
Charge of proton = e
F = (9 x 10⁹ x 54 x 1.60 x 10⁻¹⁹ x 1.60 x 10⁻¹⁹)/(4.8 x 10⁻¹⁵)²
F = 540 N
Part 3)
The mass of the proton = 1.67 x 10⁻²⁹ kg
acceleration = 540/1.67 x 10⁻²⁹
= 3.20 x 10³¹ m/s²