Mass of Copper : 63.5 g
<h3>Further explanation</h3>
Given
Reaction
Cu(s)+2AgNO₃ (aq) ⇒Cu(NO₃)₂ (aq)+2Ag(s)
Required
Mass of Copper
Solution
mol of Silver nitrate :
= M x V
= 2 mol/L x 0.5 L
= 1
From the equation, mol ratio of Cu : AgNO₃ = 1 : 2, so mol Cu = 1
Mass of Cu(Ar=63.5 g/mol) :
= mol x Ar
= 1 x 63.5
= 63.5 g
Answer:
4.4 g
Explanation:
Step 1: Write the balanced equation
Cu + 4 HNO₃ ⇒ Cu(NO₃)₂ + 2 NO₂ + 2 H₂O
Step 2: Calculate the moles corresponding to 3.2 L of NO₂ at STP
At standard temperature and pressure, 1 mole of NO₂ occupies 22.4 L.
3.2 L × 1 mol/22.4 L = 0.14 mol
Step 3: Calculate the moles of Cu needed to produce 0.14 moles of NO₂
The molar ratio of Cu to NO₂ is 1:2. The moles of Cu needed are 1/2 × 0.14 mol = 0.070 mol.
Step 4: Calculate the mass corresponding to 0.070 moles of Cu
The molar mass of Cu is 63.55 g/mol.
0.070 mol × 63.55 g/mol = 4.4 g
Explanation:
smoking is the main reason
So molarity which is represented by that 0.01M refers to the amount of moles that is present in 1L or 1dm³ of the substance, in this case the acid. Molarity refers to CONCENTRATION therefore and has little to do with the strength of the acid (the strength is dependent on the pH).
Thus your answer is OPTION B
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