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4.215 g of a metallic carbonate was heated in a hard glass tube, the CO2 evolved was found to measure 1336 mL at 27°C and 700 nm of Hg pressure. What is the equivalent weight of the metal:
Correct answer is '12.15'. Can you explain this answer?
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4.215 g of a metallic carbonate was heated in a hard glass tube, the C...
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4.215 g of a metallic carbonate was heated in a hard glass tube, the C...
Solution:
The given data are:
Mass of metallic carbonate = 4.215 g
Volume of CO2 evolved = 1336 mL
Temperature = 27°C
Pressure = 700 mm of Hg
We need to find the equivalent weight of metal.
Step 1: Calculate the number of moles of CO2 evolved
We know that,
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
Converting the given pressure and volume to SI units, we get:
P = 700 mm Hg = 93.3 kPa
V = 1336 mL = 1.336 L
T = (27 + 273) K = 300 K
R = 8.314 J/mol K
Substituting the values, we get:
n = PV/RT = (93.3 × 1.336 × 10^-3)/(8.314 × 300) = 0.0041 mol
Step 2: Calculate the molar mass of the metallic carbonate
We know that,
Molar mass = (mass of compound)/(number of moles)
Substituting the values, we get:
Molar mass = 4.215/0.0041 = 1027.7 g/mol
Step 3: Calculate the equivalent weight of the metal
We know that,
Equivalent weight = Molar mass/Valency
Valency of the metal carbonate is 2, since it contains one metal atom and two carbonate ions.
Substituting the values, we get:
Equivalent weight = 1027.7/2 = 513.85 g/equivalent
But we need to express the equivalent weight in grams per mole.
So, dividing by the Avogadro's number, we get:
Equivalent weight = 513.85/6.022 × 10^23 = 8.54 × 10^-22 g/molecule
Multiplying by 2 (since there are two metal atoms in one molecule of the metal carbonate), we get:
Equivalent weight = 1.71 × 10^-21 g/atom
Finally, multiplying by the atomic weight of the metal, we get:
Equivalent weight = 1.71 × 10^-21 × atomic weight of metal
We know that the atomic weight of the metal is approximately 196.97 g/mol (from the periodic table).
Substituting the values, we get:
Equivalent weight = 1.71 × 10^-21 × 196.97 = 3.37 × 10^-19 g/equivalent
Dividing by 2 (since there are two equivalents of metal in one molecule of the metal carbonate), we get:
Equivalent weight = 1.685 × 10^-19 g/atom
Dividing by the molar mass of the metal, we get:
Equivalent weight = 1.685 × 10^-19/196.97 = 8.54 × 10^-22 mol/atom
Finally, multiplying by the atomic weight of carbon (12.01 g/mol), we get:
Equivalent weight = 8.54 × 10^-22 × 12.01 = 1.025 × 10^-20 g/atom
Rounding off to two decimal places, we get:
Equivalent weight =
The given data are:
Mass of metallic carbonate = 4.215 g
Volume of CO2 evolved = 1336 mL
Temperature = 27°C
Pressure = 700 mm of Hg
We need to find the equivalent weight of metal.
Step 1: Calculate the number of moles of CO2 evolved
We know that,
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
Converting the given pressure and volume to SI units, we get:
P = 700 mm Hg = 93.3 kPa
V = 1336 mL = 1.336 L
T = (27 + 273) K = 300 K
R = 8.314 J/mol K
Substituting the values, we get:
n = PV/RT = (93.3 × 1.336 × 10^-3)/(8.314 × 300) = 0.0041 mol
Step 2: Calculate the molar mass of the metallic carbonate
We know that,
Molar mass = (mass of compound)/(number of moles)
Substituting the values, we get:
Molar mass = 4.215/0.0041 = 1027.7 g/mol
Step 3: Calculate the equivalent weight of the metal
We know that,
Equivalent weight = Molar mass/Valency
Valency of the metal carbonate is 2, since it contains one metal atom and two carbonate ions.
Substituting the values, we get:
Equivalent weight = 1027.7/2 = 513.85 g/equivalent
But we need to express the equivalent weight in grams per mole.
So, dividing by the Avogadro's number, we get:
Equivalent weight = 513.85/6.022 × 10^23 = 8.54 × 10^-22 g/molecule
Multiplying by 2 (since there are two metal atoms in one molecule of the metal carbonate), we get:
Equivalent weight = 1.71 × 10^-21 g/atom
Finally, multiplying by the atomic weight of the metal, we get:
Equivalent weight = 1.71 × 10^-21 × atomic weight of metal
We know that the atomic weight of the metal is approximately 196.97 g/mol (from the periodic table).
Substituting the values, we get:
Equivalent weight = 1.71 × 10^-21 × 196.97 = 3.37 × 10^-19 g/equivalent
Dividing by 2 (since there are two equivalents of metal in one molecule of the metal carbonate), we get:
Equivalent weight = 1.685 × 10^-19 g/atom
Dividing by the molar mass of the metal, we get:
Equivalent weight = 1.685 × 10^-19/196.97 = 8.54 × 10^-22 mol/atom
Finally, multiplying by the atomic weight of carbon (12.01 g/mol), we get:
Equivalent weight = 8.54 × 10^-22 × 12.01 = 1.025 × 10^-20 g/atom
Rounding off to two decimal places, we get:
Equivalent weight =
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4.215 g of a metallic carbonate was heated in a hard glass tube, the C...
Let us first determine how many mol of CO2 evolved
PV = nRT
n = PV / RT
Given data:
We need Pressure in atm., 700 mm / 760 mm = 0.921 atm
We need Volume in Liters; 1336 mL = 1.336 L
We need Temp. in Kelvins; 27 C + 273 = 300 K
R = 0.0821 L*atm / mol*K
n = (0.921 atm)(1.336 L) / (0.0821 L*atm/mol*K)(300 K) = 0.0499 moles of CO2.
Carbonate is CO3, so for every mole CO2 formed, we get 1 mol O atoms (MW = 16.00 g/mol)
Let us convert moles to a mass using 44.00 g/mol CO2. Then,
0.0499 mol CO2 * (44.00 g/mol) = 2.197g CO2.
0.0499 mol O * (16.00 g/mol) = 0.798g O atoms
So mass of carbonate lost is 2.197g + 0.798g = 2.995g
Then the original mass of the metal is, 4.215g - 2.995g = 1.220g metal.
This is the mass of metal that was equivalent to the original amount of carbonate present.
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4.215 g of a metallic carbonate was heated in a hard glass tube, the CO2 evolved was found to measure 1336 mL at 27°C and 700 nm of Hg pressure. What is the equivalent weight of the metal:Correct answer is '12.15'. Can you explain this answer?
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