Answer:
Answer D => E°(Mg°/Cu⁺²) = 0.34 + 2.37 = 2.71v
Explanation:
(Oxidation) => Mg°(s) => Mg⁺²(aq) + 2e⁻ E°(Mg°/Mg⁺²) = -2.37 v
(Reduction) => Cu⁺²(aq) + 2e⁻ => Cu°(s) E°(Cu⁺²/Cu°) = +0.34 v
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Net Rxn => Mg°(s) + Cu⁺²(aq) => Mg⁺²(aq) + Cu°(s)
Std Cell Potential (25°C/1Atm) = E°(Redn) = E°(Oxidn) = +0.34v - (-2.37v)
= 0.34v + 2.37v = 2.72v
mass defect = mass of constituents - mass of atom
N has 7p and 9n
proton mass ~ 1.00728 amu
neutron mass ~ 1.00866 amu
electron mass ~ 0.000549 amu
Nitrogen mass ~ 14.003074 amu
mass defect = (7*1.00728)-(7*1.00866)-(7*0.000549)
- 14.003074
= 0.11235amu
convert to energy, the binding energy = 1.68x10^-11 J
Answer:
Part 1:sodium
rubidium
Part 2: protons neutrons and electrons are all 12
The number of protons is equal to the no. of neutrons from the electronic arrangement of magnesium and the no. of electrons is got from the atomic no. of magnesium
CH3-CH=CH-CH2-CH3 <--------CH3-CH2-CHCl-CH2_CH3
3-Cl-pentane , 3-Hal-pentane
Answer: B) 46.7% Si and 53.3% O
Explanation:
To calculate the mass percent of element in a given compound, we use the formula:
Mass of quartz 
= 5.05 g
Mass of silicon = 2.36 g
Mass of oxygen = Mass of quartz - mass of silicon = 5.05g - 2.36 g = 2.69 g
Thus the percentages of silicon and oxygen in quartz are B) 46.7% Si and 53.3% O
