1 mole Cu ------------------ 6.02x10²³ atoms
0.90 moles Cu ------------ ??
0.90 x ( 6.02x10²³ ) / 1 =
= 5.41x10²³ atoms
Answer:
sublime, melt, condense, deposit
Explanation:
1. When ice is warmed at a steady pressure 0.00512 atm, it will be sublime.
2. It will be melt when ice is warmed at a consistent pressure of 1 atm.
3. If water vapour pressure is continued to increase at a temperature of 100 C, it will be condense.
4. If water vapour pressure is continued to increase at a temperature of -50 C, it will be deposited.
Answer: A) Ar
Explanation: Argon [Ar] has an atomic no of 18 and the electronic configuration is:
Ar :
Chlorine [Cl] has atomic no of 17 and thus the electronic configuration is :
Cl :
Magnesium [Mg] has atomic no of 12 and thus the electronic configuration is :
Mg :
Sodium has atomic no of 11 and thus the electronic configuration is :
Cl :
As we move across a period the number of electrons are being added to the same shell but the number of protons increases, thus the electrons are being tightly held and thus the atomic radius keeps on decreasing.
Thus the smallest atom would have a tightly bound electron nearer to the nucleus. As argon is the last element of the period, it is the smallest in the period and thus largest amount of energy will be required to remove the outermost electron.
<h3>Answer:</h3>
SALT
<h3>Explanation:</h3>
Salt is formed by the opposite ions bonded to each other through Ionic Bond. The two ions i.e. Cation and Anions are formed by oxidation and reduction reactions respectively. General dissociation of salt is represented as,
MN → Mⁿ⁺ + Nⁿ⁻
where;
Mⁿ⁺ = Cation
Nⁿ⁻ = Anion
MN = Salt
Following is the list of salts which when when dissociates produces Cations and Anions other than OH⁻ (Hydroxide) and H⁺ (Hydrogen Ion).
Magnesium Sulfate:
MgSO₄ → Mg²⁺ + SO₄²⁻
Sodium Chloride:
NaCl → Na⁺ + Cl⁻
Sodium Carbonate:
Na₂CO₃ → 2 Na⁺ + CO₃²⁻
Ammonium Dichlorate:
(NH₄)₂Cr₂O₇ → 2 NH₄⁺ + Cr₂O₇²⁻
Answer:
81% Yield
Explanation:
2CO + O₂ => 2CO₂
Excess 3.70g O₂ => 8.25g CO₂ (actural yield)
(3.70g O₂)/(32g O₂/mol O₂)
= 0.1156 mol O₂ => 2(0.1156) mol CO₂
= 10.175g (Theoretical Yield)
%Yield = (Actual Yield / Theoretical Yield)100%
= (8.25g/10.175g)100% = 81% Yield
