A mass of 5.4 grams of aluminum (al) reacts with an excess of copper (ii) chloride (cucl2) in solution, as shown below. 3cucl2 2

The epicenter is determined to be located on a circle that is centered around Recording station X, with a radius extending 250 km.

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.

To solve for density, you can use the formula--> Density= PM/ RT, where P stands for pressure, M for molar mass, R represents the gas constant, and T is temperature. 

P= 1.75 atm
M= 16.01 g/ mol
R= 0.0821 atm·L/ mol·K
T=337 k

Thus, the density calculation becomes: density= (1.75 x 16.01)/ (0.0821 x 337)= 1.01 g/L

The quantity of fluorine in moles is calculated as 71/19 = 3.74
We also know that at standard temperature and pressure (273 K and 101.3 kPa), one mole of gas occupies 22.4 liters
So, the volume for 3.74 moles at S.T.P is: 3.74 x 22.4
This results in a volume of 83.776 L, which is equivalent to 83,776 mL

Next, applying Boyle's law, which states that for a fixed amount of gas,
PV = constant

We set up the equation P x 6843 = 101.3 x 83776
Solving for P gives us 1,240 kPa

Answer: Reaction 2 is a spontaneous one.

Explanation:

According to our understanding:

= +ve, meaning the reaction is non-spontaneous

= -ve, indicating the reaction is spontaneous

= 0, stating that the reaction is at equilibrium

For a reaction to be classified as spontaneous, the Gibbs free energy must yield a negative value.

Reaction 1:

Glucose + Pi ⟶ glucose-6-phosphate + H₂O, ΔG = +13.8 kJ/mol

Reaction 2:

ATP + H₂O ⟶ ADP + Pi, ΔG = -30.5 kJ/mol

From this, we can conclude that ΔG being negative indicates that reaction 2 is indeed spontaneous.