What mas of liquid mercury should be produced by the reaction between 5.0 mL of 0.1102 M mercury(II)nitrate ans 0.621 grams of silver metal?
would the formula be...
Hg(NO3)2(aq) + 2Ag(aq)--> 2AgNO3(aq) + Hg(l)
Look at the limiting reagent problem you posted just above. This is worked the same way. Your equation looks ok.
Yes, the balanced chemical equation for the reaction between mercury(II) nitrate and silver metal is:
Hg(NO3)2(aq) + 2Ag(s) → 2AgNO3(aq) + Hg(l)
To determine the mass of liquid mercury produced, we need to follow these steps:
Step 1: Convert the volume of mercury(II) nitrate solution to moles.
Given: Volume of mercury(II) nitrate = 5.0 mL = 0.0050 L
Molarity of mercury(II) nitrate = 0.1102 M
To convert from volume (in liters) to moles, we use the formula:
moles = volume (L) × concentration (M)
moles of Hg(NO3)2 = 0.0050 L × 0.1102 M = 0.000551 moles
Step 2: Convert the mass of silver to moles.
Given: Mass of silver = 0.621 grams
Molar mass of silver (Ag) = 107.87 g/mol
To convert from grams to moles, we use the formula:
moles = mass (g) / molar mass (g/mol)
moles of Ag = 0.621 g / 107.87 g/mol = 0.00576 moles
Step 3: Determine the limiting reagent.
To determine which reactant is the limiting reagent, we compare the mole ratio of the reactants from the balanced equation.
From the balanced equation, the mole ratio of Hg(NO3)2 to Ag is 1:2. This means that 1 mole of Hg(NO3)2 reacts with 2 moles of Ag.
Using the moles calculated in Step 1 and Step 2, we can compare the moles based on the mole ratio:
moles of Hg(NO3)2 : moles of Ag = 0.000551 : 0.00576
Since the ratio of moles is less than 1:2, it means that Hg(NO3)2 is the limiting reagent.
Step 4: Convert moles of limiting reagent to moles of Hg.
From the balanced equation, we know that the mole ratio of Hg(NO3)2 to Hg is 1:1.
moles of Hg = 0.000551 moles
Step 5: Convert moles of Hg to mass of Hg.
Molar mass of Hg = 200.59 g/mol
mass of Hg = moles of Hg × molar mass of Hg
mass of Hg = 0.000551 mol × 200.59 g/mol = 0.110 g
Therefore, the mass of liquid mercury produced by the reaction is 0.110 grams.