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2 years ago

Calculate the mole fraction of the ionic species kcl in the solution.

Chemistry

1 answer:

sp2606 [1]2 years ago

8 0

The question is incomplete, here is the complete question:

Calculate the mole fraction of the ionic species KCl in the solution A solution was prepared by dissolving 43.0 g of KCl in 225 g of water.

Answer: The mole fraction of KCl in the solution is 0.044

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For water:

Given mass of water = 225 g

Molar mass of water = 18 g/mol

Putting values in equation 1, we get:

$\text{Moles of water}=\frac{225g}{18g/mol}=12.5mol$

For KCl:

Given mass of KCl = 43 g

Molar mass of KCl = 74.55 g/mol

Putting values in equation 1, we get:

$\text{Moles of KCl}=\frac{43g}{74.55g/mol}=0.577mol$

Mole fraction of a substance is given by:

$\chi_A=\frac{n_A}{n_A+n_B}$

For KCl:

Moles of KCl = 0.577 moles

Total moles = [0.577 + 12.5] = 13.077 moles

Putting values in above equation, we get:

$\chi_{(KCl)}=\frac{0.577}{13.077}=0.044$

Hence, the mole fraction of KCl in the solution is 0.044

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How many grams N2F4 can be produced from 225 g F,?

zavuch27 [327]

Answer:

308 g

Explanation:

Data given:

mass of Fluorine (F₂) = 225 g

amount of N₂F₄ = ?

Solution:

First we look to the reaction in which Fluorine react with Nitrogen and make N₂F₄

Reaction:

2F₂ + N₂ -----------> N₂F₄

Now look at the reaction for mole ratio

2F₂ + N₂ -----------> N₂F₄

2 mole 1 mole

So it is 2:1 mole ratio of Fluorine to N₂F₄

As we Know

molar mass of F₂ = 2(19) = 38 g/mol

molar mass of N₂F₄ = 2(14) + 4(19) =

molar mass of N₂F₄ = 28 + 76 =104 g/mol

Now convert moles to gram

2F₂ + N₂ -----------> N₂F₄

2 mole (38 g/mol) 1 mole (104 g/mol)

76 g 104 g

So,

we come to know that 76 g of fluorine gives 104 g of N₂F₄ then how many grams of N₂F₄ will be produce by 225 grams of fluorine.

Apply unity formula

76 g of F₂ ≅ 104 g of N₂F₄

225 g of F₂ ≅ X of N₂F₄

Do cross multiplication

X of N₂F₄ = 104 g x 225 g / 76 g

X of N₂F₄ = 308 g

So,

308 g N₂F₄ can be produced from 225 g F₂

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2 years ago

What type of reaction is shown in this thermochemical equation? A + B + heat → C + D

hodyreva [135]

The reaction, as what is depicted in the thermonuclear equation is one of the best example of an endothermic reaction. In addition, the endothermic process revolves around the idea that the system can also absorb the energy from its surroundings, in contrast to the idea of releasing its energy to its environment.

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2 years ago

Read 2 more answers

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction:P4(g) + 10 Cl2(g) → 4PCl5(s) ΔH°

miskamm [114]

Answer: The $\Delta H^o_{rxn}$ for the reaction is -1835 kJ.

Explanation:

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction follows:

$P_4(g)+10Cl_2(g)\rightarrow 4PCl_5(s)$ $\Delta H^o_{rxn}=?$