Answer:
<em><u>Mass of Ni = 4.14 grams</u></em>
Explanation:
Molar mass : It is the amount of substance present in 1 mole of the molecules.
Moles : It is the quantity that contains as many atoms as present in 12 gram of C-12. This is equal to Avogadro Number .
Molar mass of Ni = 58.69 g/mole
Moles can be calculated by two formula:
........(1)
And ,
.........(2)
Comparing equation 1 and 2
M = 58.69 g/mole
Put these value in the formula and solve for m
m = 4.14 gram
<em><u>Mass of Ni = 4.14 grams</u></em>
<em><u>Second Approach :</u></em>
Find the moles first using :
Then put value of n in the formula(1) and solve for m
........(1)
Answer:We want the enthalpy associated with the reaction.........
Explanation:
H
3
CCH
2
OH
(
l
)
+
Δ
→
H
3
CCH
2
OH
(
g
)
You have a mass of
50.0
⋅
g
EtOH
, that is assumed to be at
78.3
∘
C
, and the enthalpy of vaporization is calculated by the product:
Δ
H
∘
vaporization
=
50.0
⋅
g
46.07
⋅
g
⋅
m
o
l
−
1
×
38.6
⋅
k
J
⋅
m
o
l
−
1
=
Explanation:
Answer:
0.07906687 amu
Explanation:
For Boron ₅B¹¹, the number of protons is 5 and the mass is 11. The mass is the number of protons plus the number of neutrons, so:
neutrons = 11 - 5 = 6
The mass of an atom is concentrated in the nucleus, so it is the mass of the protons + the mass of the neutrons. The mass of 1 proton is 1.00727647 amu/proton, and the mass of 1 neutron: 1.00866492 amu/neutron, so for the element given the theoretical mass (mt) is:
mt = 5* 1.00727647 amu/proton + 6*1.00866492 amu/neutron
mt = 11.08837187 amu
The mass defect (md) is the theorical mass less the real mass:
md = 11.08837187 - 11.009305
md = 0.07906687 amu
