Answer:
8.37 grams
Explanation:
The balanced chemical equation is:
C₆H₁₂O₆ ⇒ 2 C₂H₅OH (l) + 2 CO₂ (g)
Now we are asked to calculate the mass of glucose required to produce 2.25 L CO₂ at 1atm and 295 K.
From the ideal gas law we can determine the number of moles that the 2.25 L represent.
From there we will use the stoichiometry of the reaction to determine the moles of glucose which knowing the molar mass can be converted to mass.
PV = nRT ⇒ n = PV/RT
n= 1 atm x 2.25 L / ( 0.08205 Latm/kmol x 295 K ) =0.093 mol CO₂
Moles glucose required:
0.093 mol CO₂ x ( 1 mol C₆H₁₂O₆ / 2 mol CO₂ ) = 0.046 mol C₆H₁₂O₆
The molar mass of glucose is 180.16 g/mol, then the mass required is
0.046 mol x 180.16 g/mol = 8.37 g
Dalton thought that atoms were indivisible particles. But Thomsons discovery of the electron proved that the subatomic particles exist.
Divide the mass of the compound in grams by the molar mass you just calculated. The answer is the number of moles of that mass of compound.
I hope it helps
Answer is: volume of the sample is 36,2 mL.
V₁(sample) = 17 mL.
T₁(sample) = −112°C = -112 + 273,15 = 161,15 K.
T₂(sample) = 70°C = 70 + 273,15 = 343,15 K.
V₂(sample) = ?
Charles' Law: V₁/T₁ = V₂/T₂.
17 mL/161,15 K = V₂/343,15 K.
161,15 K · V₂ = 17 mL · 343,15 K
V₂ = 5833,55 K·mL ÷ 161,15 K
V₂ = 36,2 mL.
Answer:
Covalent bonds are intramolecular bonds whereas hydrogen bonds are intermolecular bonds.
<u>hope this helps and good luck :)</u>
