An element consists of 1.40% of an isotope
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Answer:
0.4076 g
Explanation:
Kp is the equilibrium constant based on pressure and depends only on gas substances. For a generic reaction
aA + bB ⇄ cC + dD
, where pX is the pressure of X in equilibrium.
For the reaction Kp = pCO₂
pCO₂ = 0.026 atm
The system is in equilibrium at the beginning. The compression occurs at a constant temperature, so using Boyle's law
P1V1 = P2V2
0.026*10 = P2*0.1
P2 = 2.6 atm
The reaction will reach again the equilibrium, and pCO₂ = 0.026 atm, then the rest will form MgCO₃, which will be 2.6 - 0.026 = 2.574 atm.
By the ideal gas law:
PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.082 atm*L/mol*K), and T is the temperature.
2.574*0.1 = n*0.082*650
53.3n = 0.2574
n = 4.83x10⁻³ mol
The stoichiometry of the reaction is 1 mol of MgCO₃ for 1 mol of CO₂, so it will form 4.83x10⁻³ mol of MgCO₃ .
The molar mass is:
MgCO₃: 24 g/mol of Mg + 12 g/mol of C + 3*16 g/mol of O = 84 g/mol
The mass formed is the molar mass multiplied by the number of moles:
m = 84x4.83x10⁻³
m = 0.4076 g
The mass of nitric acid (HNO₃) required for the production of 2.8 g of nitroglycerin? (C₃H₅N₃O₉) is 2.33 g
We'll begin by calculating the mass of HNO₃ that reacted and the mass of C₃H₅N₃O₉ produced from the balanced equation. This can be obtained as follow:
C₃H₈O₃ + 3HNO₃ —> C₃H₅N₃O₉ + 3H₂O
Molar mass of HNO₃ = 1 + 14 + (16×3)
= 1 + 14 + 48
= 63 g/mol
Mass of HNO₃ from the balanced equation = 3 × 63 = 189 g
Molar mass of C₃H₅N₃O₉ = (12×3) + (1×5) + (14×3) + (16 × 9)
= 36 + 5 + 42 + 144
= 227 g/mol
Mass of C₃H₅N₃O₉ from the balanced equation = 1 × 227 = 227 g
<h3>SUMMARY:</h3>From the balanced equation above,
227 g of C₃H₅N₃O₉ were produced by 189 g of HNO₃.
Finally, we shall determine the mass of HNO₃ that will produce 2.8 g of C₃H₅N₃O₉. This can be obtained as follow:
From the balanced equation above,
227 g of C₃H₅N₃O₉ were produced by 189 g of HNO₃.
Therefore,
2.8 g of C₃H₅N₃O₉ will be produce by = = 2.33 g of HNO₃
Thus, the mass of nitric acid (HNO₃) required for the production of 2.8 g of nitroglycerin? (C₃H₅N₃O₉) is 2.33 g
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