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storchak [24]
3 years ago
7

The properties of two elements are listed below. Element Atomic radius (pm) Ionic radius (pm) First ionization energy (kJ/mol) E

lectron affinity (kJ/mol) Electronegativity Br 114 195 1140 –325 3.0 K 243 152.2 418.8 –48.4 0.82 Which prediction is supported by the information in the table? K will give up an electron more easily than Br. Both K and Br will have the same pull on electrons. K will have a smaller size in comparison to Br. Both K and Br will produce ions of the same size.
Chemistry
1 answer:
Sedbober [7]3 years ago
5 0

Answer:

K will give up an electron more easily than Br.

Explanation:

Electronegativity of an element is a property that combines the ability of its atom to lose and gain electrons.

The lower the electronegativity value, the more electropositive an element is and the more readily it loses electrons.

From the data given, we see that Br has an E.N value of 3.0 and K has an E.N value of 0.82.

Therefore, Br is highly electronegative and it is able to attract electrons to itself whereas K has a low E.N value. K will give up electrons more readily.

Lookinf at other information in the table, the larger atomic radius and lower ionizaton energy of K are all pointers to how readily it would be able to lose electrons.

We can conclude that K is even a metal.

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<u>Answer:</u> The final pressure in the vessel will be 0.965 atm

<u>Explanation:</u>

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

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

  • <u>For phosphorus trichloride:</u>

Given mass of phosphorus trichloride = 20.0 g

Molar mass of phosphorus trichloride = 137.3 g/mol

Putting values in equation 1, we get:

\text{Moles of phosphorus trichloride}=\frac{20.0g}{137.3g/mol}=0.146mol

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Given mass of oxygen gas = 3.15 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

\text{Moles of oxygen gas}=\frac{3.15g}{32g/mol}=0.098mol

The chemical equation for the reaction of phosphorus trichloride and oxygen gas follows:

2PCl_3+O_2\rightarrow 2POCl_3

By Stoichiometry of the reaction:

2 moles of phosphorus trichloride reacts with 1 mole of oxygen gas

So, 0.146 moles of phosphorus trichloride will react with = \frac{1}{2}\times 0.146=0.073mol of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.

Thus, phosphorus trichloride is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of phosphorus trichloride produces 2 moles of POCl_3

So, 0.146 moles of phosphorus trichloride will produce = \frac{2}{2}\times 0.146=0.146mol of POCl_3

To calculate the pressure of the vessel, we use the equation given by ideal gas follows:

PV=nRT

where,

P = pressure of the vessel = ?

V = Volume of the vessel = 6.00 L

T = Temperature of the vessel = 210^oC=[210+273]K=483K

R = Gas constant = 0.0821\text{ L. atm }mol^{-1}K^{-1}

n = number of moles = 0.146 moles

Putting values in above equation, we get:

P\times 6.00L=0.146mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 483K\\\\P=\frac{0.146\times 0.0821\times 483}{6.00}=0.965atm

Hence, the final pressure in the vessel will be 0.965 atm

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