Find the empirical formula of each of the following compounds. Given mass or for each element in a sample of the compound 3,611

Answer: refer to the explanation

Explanation:

This question requires calculating mass. To determine the mass, we need values for two parameters, namely the specifications for the grade 70 tow chain and the mass per unit length given.

Assuming the mass per unit length is 3 kilograms per meter (kg/m) and the length of the grade 70 tow chain is 5 meters (m).

Thus, the formula used to compute the mass of the chain is as follows;

Mass of the chain = mass per unit length (kg/m) × length ---------------------------------------------------------------------------------------------------------------------(1).

Mass of the chain = 3 kg/m × 5 m.

Mass of the chain equals 15 kg.

The percentage of KCl present in the mixture is approximately <span>40%</span><span>If we consider a 100-gram sample of the mixture:ω(K) = 44.20% ÷ 100% = 0.442.
m(K) = 0.442 · 100 g = 44.2 g.</span>n(K) = 44.2 g ÷ 39.1 g/mol.
n(K) = 1.13 mol.
n(KCl) + n(KNO₃) = n(K)
m(KCl) = x.
m(KNO₃) = y.
Two equations:
1) x + y = 100 g.
2) m(KCl)/M(KCl) + m(KNO₃)/M(KNO₃) = 1.13 mol.
x/74.55 g/mol + y/101.1 g/mol = 1.13 mol.
From the first equation, we find x = 100 - y and substitute into the second equation:
(100 - y)/74.55 + y/101.1 = 1.13 /×101.1.
135.61 - 1.356y + y = 114.24.
0.356y = 22.37 g.
y = 62.83 g.
Thus, x = m(KCl) = 100 g - 62.83 g = 37.17 g.

Answer: The vapor pressure of naphthalene within the flask remains at atm.

Explanation:

The transformation from solid naphthalene to its gaseous form follows the equilibrium reaction:

• The formula employed to determine the enthalpy change for the reaction is:  

The formula for calculating the enthalpy change regarding the aforementioned reaction is:

The provided information includes:

Substituting the values into the previous equation produces:

• The formula utilized to compute Gibbs free energy change is of a reaction:

The equation for the enthalpy change for the reaction is:

The given factors include:

By inserting values from the above equation, we arrive at:

• For the calculation of (at 25°C) regarding the provided value of Gibbs free energy, the following relationship is applied:

where,

= Gibbs free energy = 22.5 kJ/mol = 22500 J/mol  (Conversion factor: 1kJ = 1000J)

R = Gas constant =

T = temperature =

= equilibrium constant at 25°C =?

Inserting values into the above equation yields:

• To determine the equilibrium constant at 35°C, we refer to the equation proposed by Arrhenius, which states:

where,

= Equilibrium constant at 35°C =?

= Equilibrium constant at 25°C =

= Enthalpy change of the reaction = 72.1 kJ/mol = 72100 J

R = Gas constant =

= Initial temperature =

= Final temperature =

By plugging values into the equation above, we obtain:

• In order to calculate the partial pressure of naphthalene at 35°C, we utilize the equation for , which is:

The partial pressure of the solid phase is considered to be 1 at equilibrium.

Therefore, the value for will equal

Consequently, the partial pressure of naphthalene at 35°C is atm.

Utilize the ideal gas law:

n = PV / RT

P = 100kPa = 100 x 1000 x (9.8 x 10^{-6}) = 0.98 atm
Convert kPa to atm, where 1 Pa = 9.8 x 10^{-6} atm.
T = 293 K
V = 6.8 L
R = 1/12
Substituting all values leads to:
n = 0.272

I expect the product's mass to be 400 grams. This belief stems from the law of conservation of mass, which states that mass can neither be created nor destroyed. In a sealed system, the mass of the reactants equals the mass of the products. Therefore, since the total mass of the reactants is 400 grams, the resulting mass of the products must also be 400 grams

OR

200