Leonard adds 5 grams of sugar to 1 liter of water to make one sugar solution. Then he adds 10 grams of sugar to 1 liter of water

Answer:

The right answer is "1.0100".

Explanation:

Assuming the total volume of the mixture is 100 ml.

Thus,

The volume of DMSO will be 10 mL and the volume of water will be 90 mL.

For DMSO:

=

=

The total mass of the mixture will be:

=

=

Calculating the density of the mixture:

=

=

=

Thus,

The specific gravity of the mixture is:

=

=

=

Mole fraction of oxygen gas: 0.381

Additional clarification

Given:

2.31 atm Oxygen

3.75 atm Hydrogen

Required:

Mole fraction of Oxygen

Calculation:

According to Dalton’s Law of partial pressures

P tot = P₁ + P₂ +.. + Pₙ

Substituting values:

P tot = P O₂ + P H₂

P tot = 2.31 atm + 3.75 atm

P tot = 6.06 atm

Mole fraction of O₂ (X O₂):

P O₂ = X O₂ x P tot

X O₂ = P O₂ / P tot

X O₂ = 2.31 / 6.06

X O₂ = 0.381

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Answer:

The response is provided below.

Explanation:

Numerous aspects can influence the actual results of titration. These factors vary from human error to misjudging measurements, a researcher's interpretation of color changes, and improper techniques during the experimental procedure.

Thus, to mitigate these errors, researchers must engage thoroughly throughout experimentation, and employing gross readings can assist in reducing mistakes when determining the final titre value.

Answer:

Complete Question:  

Equimolar quantities of CH3OH(l) and C2H5OH(l) are placed in separate 2.0 L containers that have been evacuated beforehand. Pressure gauges are attached to each container, and the temperature is maintained at 300 K. In both containers, liquid is consistently visible at the bottom. The varying pressure within the vessel that contains CH3OH(l) is illustrated below.

In comparison to the equilibrium vapor pressure of CH3OH(l) at 300 K, the equilibrium vapor pressure of C2H5OH(l) at 300 K is

ANSWER : lower, since the London dispersion forces among C2H5OH molecules surpass those among CH3OH molecules.

Explanation:

To clarify the answer provided, let’s begin by defining some concepts.

The London dispersion force is the least strong type of intermolecular force. It is a temporary force that arises when the electron arrangement in two neighboring atoms creates transient dipoles.  

The vapor pressure of a liquid reflects the equilibrium pressure of its vapor above the liquid (or solid); specifically, it represents the pressure associated with the evaporation of a liquid (or solid) in a sealed environment above the substance.

The pressure will be lower due to the stronger London dispersion forces acting between C2H5OH molecules compared to those between CH3OH molecules. This implies that when intermolecular forces are stronger, they intensify the interactions binding the substance together, thereby reducing the liquid's vapor pressure at any given temperature and making it more difficult to vaporize the substance.

Note: The London dispersion force for C2H5OH is more substantial than for CH3OH because C2H5OH has more electrons than CH3OH.