Answer:
The initial volume of Ne gas is 261mL
Explanation:
This question can be answered using Ideal Gas Equation;
However, the following are the given parameters
Initial Pressure = 654mmHg
Finial Pressure = 345mmHg
Final Volume = 495mL
Required
Initial Volume?
The question says that Temperature is constant;
This implies that, we'll make use of Boyle's law ideal gas equation which states;
Where 
represent the initial pressure
represent the final pressure
represent the initial temperature
represent the final temperature
Substitute these values in the formula above;
Divide both sides by 654
(Approximated)
<em>The initial volume of Ne gas is 261mL</em>
Answer:
a) both substances are insoluble in water
b) both substances are soluble in ligroin
c) both substances suffer combustion, octane produces more CO₂ than hexene.
d) both substances are less dense than waterl, with hexene having the lowest density.
e) only hexene would react with bromine
f) only hexene would react with permanganate
Explanation:
a) both substances are non-polar and water is polar
b) both substances are non-polar and lingroin is non-polar
c) C₈H₁₈ + 17.5O₂ → 8CO₂ + 9H₂O
C₆H₁₂ + 9O₂ → 6CO₂ + 6H₂O
d) water = 997 kg/m³
ocatne = 703 kg/m³
hexene = 673 kg/m³
e) bromine test is used to detect unsaturations
f) permanganate test is used to detect unsaturations
Answer:second law of thermodynamics
Explanation:the second law of thermodynamics states that the total entropy of an isolated system can never decrease over time and is constant if only if all processes are reversible.
Answer:
A. The partial pressure for CH4 = 0.0925atm
B. The partial pressure for C2H6 = 0.925atm
C. The partial pressure for C3H8 = 0.346atm
D. The partial pressure for C4H10 = 0.115atm
Explanation:
Total pressure = 1.48atm
Total mole = 0.4+4+1.5+0.5=6.4
A. Mole fraction of CH4 = 0.4/6.4 = 0.0625
The partial pressure for CH4 = 0.0625 x 1.48 = 0.0925atm
B. Mole fraction of C2H6 = 4/6.4 = 0.625
The partial pressure for C2H6 = 0.625 x 1.48 = 0.925atm
C. Mole fraction of C3H8 = 1.5/6.4 = 0.234
The partial pressure for C3H8 = 0.234 x 1.48 = 0.346atm
D. Mole fraction of C4H10 = 0.5/6.4 = 0.078
The partial pressure for C4H10 = 0.078 x 1.48 = 0.115atm
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