3Cu + 8HNO = 3Cu(NO3)2 +2NO + 4H2O
1 answer:
Taking into account the reaction stoichiometry, 5.2634 grams of Cu(NO₃)₂ are formed when 4.69 grams of HNO₃, assuming an excess of solid copper is present.
<h3>Reaction stoichiometry</h3>In first place, the balanced reaction is:
3 Cu+ 8 HNO₃ → 3 Cu(NO₃)₂ + 2 NO + 4 H₂O
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- Cu: 3 moles
- HNO₃: 8 moles
- Cu(NO₃)₂: 3 mole
- NO: 2 moles
- H₂O: 4 moles
The molar mass of the compounds is:
- Cu: 63.55 g/mole
- HNO₃: 63 g/mole
- Cu(NO₃)₂: 187.55 g/mole
- NO: 30 g/mole
- H₂O: 18 g/mole
Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
- Cu: 3 moles ×63.55 g/mole= 190.65 grams
- HNO₃: 8 moles ×63 g/mole= 504 grams
- Cu(NO₃)₂: 3 moles ×187.55 g/mole= 562.65 grams
- NO: 2 moles ×30 g/mole= 60 grams
- H₂O: 4 moles ×18 g/mole= 72 grams
The following rule of three can be applied: if by reaction stoichiometry 504 grams of HNO₃ form 562.65 grams of Cu(NO₃)₂, 4.69 grams of HNO₃ form how much mass of Cu(NO₃)₂?
<u><em>mass of Cu(NO₃)₂= 5.2634 grams</em></u>
Then, 5.2634 grams of Cu(NO₃)₂ are formed when 4.69 grams of HNO₃, assuming an excess of solid copper is present.
Learn more about the reaction stoichiometry:
#SPJ1
You might be interested in
Answer:
1. Molarity of MgSO₄ = 0.6 M
2. Molarity of AgNO₃ = 0.06 M
3. volume of acetic acid = 250 mL
4. Molarity of NaCl= 2.3 M
5. Mass of C₁₂H₂₂O₁₁ = 4.1 g
6. Mass of C₁₀H₈ (naphthalene) = 77 g
7. mass of ethanol = 11 g
8. Mass of DDT = 0.011 mg
Explanation:
Ans 1.
Data given
mass of MgSO₄ = 403
Volume of solution = 5.25 L
Solution:
First we will find mole of solute
no. of moles = mass in grams / Molar mass . . . . . .(1)
Molar mass of MgSO₄ = 24 + 32 + 4(16)
Molar mass of MgSO₄ = 120 g/mol
Put values in equation 1
no. of moles = 403 g / 120 g/mol
no. of moles = 3.36 mol
Now to find molarity
Formula used
Molarity = No. of moles of solute / solution in L . . . . . . (2)
Put Values in above equation
M = 3.36 mol / 5.25 L
M = 0.64
So, round the figure to two significant digits.
Molarity of MgSO₄ = 0.64 M
_____________________
Ans 2.
Data given
mass of AgNO₃ = 1.24 g
Volume of solution = 125 mL
convert mL to L
1000 mL = 1 L
125 mL = 125/1000 = 0.125
Solution:
First we will find mole of solute
no. of moles = mass in grams / Molar mass . . . . . .(1)
Molar mass of AgNO₃ = 108 + 14 + 3(16)
Molar mass of AgNO₃ = 170 g/mol
Put values in equation 1
no. of moles = 1.24 g / 170 g/mol
no. of moles = 0.0073 mol
Now to find molarity
Formula used
Molarity = No. of moles of solute / solution in L . . . . . . (2)
Put Values in above equation
M = 0.0073 mol / 0.125 L
M = 0.06
So, round the figure to two significant digits.
Molarity of AgNO₃ = 0.06 M
______________________
Ans 3.
Data Given:
volume of acetic acid = 500 mL
% solution of acetic acid (M)= 50%
volume of acetic acid needed = ?
Solution:
formula used
percent of solution = volume of solute/ volume of solution x 100
Put Values in above formula
50 % = volume of solute / 500 mL x 100
Rearrange the above equation
volume of solute = 50 x 500 mL /100
volume of solute = 250 mL
So, volume of acetic acid = 250 mL
______________________
Ans 4
Data Given:
Molarity of NaCl (M1) = 6 M
Volume of NaCl (V1) = 750 mL
convert mL to L
1000 ml = 1 L
750 ml = 750/1000 = 0.75 L
Volume of dilute solution (V2)= 2 L
Molarity of dilute solution (M2) = ?
Solution:
Dilution Formula will be used
M1V1 = M2V2 . . . . . . (1)
Put values in equation 1
6 M x 0.75 L = M2 x 2 L
Rearrange the above equation
M2 = 6 M x 0.75 L / 2 L
M2 = 2.25 M
So, round the figure to two significant digits.
Molarity of NaCl= 2.3 M
_________________________
Ans 5.
Data Given:
Molarity of C₁₂H₂₂O₁₁ = 0.16 M
Mass of C₁₂H₂₂O₁₁ (m) = ?
Volume of dilute solution = 75 mL
convert mL to L
1000 ml = 1 L
75 ml = 75/1000 = 0.075 L
Solution:
As we know
Molarity = no.of moles/ liter of solution . . . . . . .(1)
we also know that
no.of moles = mass in grams / molar mass . . . . . (2)
Combine both equation 1 and 2
Molarity = (mass in grams / molar mass) / liter of solution . . . . (3)
Molar mass of C₁₂H₂₂O₁₁ (Sucrose) = 12(12) +22(1) +11(16)
Molar mass of C₁₂H₂₂O₁₁ (Sucrose) = 144 +22 + 176
Molar mass of C₁₂H₂₂O₁₁ (Sucrose) = 342 g/mol
Put values in equation in equation 3
0.16 M = (mass in grams / 342 g/mol) / 0.075 L
Rearrange the above equation
mass in grams = 0.16 mol/L x 0.075 L x 342 g/mol
mass in grams = 4.104 g
So, round the figure to two significant digits.
Mass of C₁₂H₂₂O₁₁ = 4.1 g
____________________
The remaing portion is in attachment
