CHEMISTRY HIGH SCHOOL

At equilibrium, a sample of gas from the system is collected into a 4.00 L flask at 600 K. The flask is found to contain 3.86 g of PCl₅, 12.7 g of PCl₃, and 13.3 g of Cl₂. What are the values of Kc and Kp for this reaction?

Answers

Answer 1

Answer:

Answer:

Explanation:

PCl₅ ⇄ PCl₃ + Cl₂

1 mole 1 mole 1 mole

molecular weight of PCl₅ = 208.5

molecular weight of PCl₃ = 137.5

molecular weight of Cl₂ = 71

moles of PCl₅ = .0185

moles of PCl₃ = .0924

moles of Cl₂ = .1873

Total moles = .2982 moles

mole fraction of PCl₅ = .062

mole fraction of PCl₃ = .31

mole fraction of Cl₂ = .628

If total pressure be P

partial pressure of PCl₅ = .062 P

partial pressure of PCl₃ = .31 P

partial pressure of Cl₂ = .628 P

Kp = .31 P x .628 P / .062 P

= 3.14 P

To calculate Total pressure P

PV = nRT

P x 4 x 10⁻³ = .2982 x 8.31 x 600

P = 371.7 x 10³

= 3.717 x 10⁵ Pa

Kp = 3.14 P = 3.14 x 3.717 x 10⁵ Pa

= 11.67 x 10⁵ Pa

Kp = Kc x $( RT )^(\triangle n)$

$\triangle n$ = 1

11.67 x 10⁵ = Kc x $( 8.31* 600 )^(1)$

Kc = 234

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What is the formula of the ion formed when potassium achieves noble-gas electron configuration

Answers

Answer;

K+

Explanation;

-Noble gas configuration is the electron configuration equivalent to noble gases or group 8 elements. According to the octet rule an atom of an element gains or looses electrons to attain noble gases configuration which is the stable configuration, such that an atom has attained maximum number of electrons in the outermost energy level.

-For instance potassium is an alkali metal, consisting of one valence electron in the outermost energy level. For an atom of potassium to attain octet configuration or noble gases configuration it will have to loose one electron, thus forming a positively charged ion of potassium, K+.

potassium is an alkali metal which means that it only needs to get rid of one electron to achieve a noble gas configuration. Since it only needs to get rid of one electron the ion will be a cation with a charge of +1 which means the symbol will be K⁺.

I hope this helps. Let me know if anything is unclear.

The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell:________ Pt(s)
|H2(g,1atm)
|H+(aq,1.0M)
|Au3+(aq,?M)
|Au(s).
What is the concentration of Au3+ in the solution if Ecell is 1.23 V ?

Answers

Answer: The concentration of $Au^(3+)$ is $1.096* 10^(-6)$

Explanation:

The given chemical cell follows:

$Pt(s)|H_2(g,1atm)|H^+(aq,1.0M)||Au^(3+)(aq,?M)|Au(s)$

Oxidation half reaction: $H_2(g,1atm)\rightarrow 2H^(+)(aq,1.0M)+2e^-;E^o_(2H^(+)/H_2)=0.0V$ ( × 3)

Reduction half reaction: $Au^(3+)(aq,?M)+3e^-\rightarrow Au(s);E^o_(Au^(3+)/Au)=1.50V$ ( × 2)

Net cell reaction: $3H_2(g,1atm)+2Au^(3+)(aq,?M)\rightarrow 6H^(+)(aq,1.0M)+2Au(s)$

Oxidation reaction occurs at anode and reduction reaction occurs at cathode.

To calculate the $E^o_(cell)$ of the reaction, we use the equation:

$E^o_(cell)=E^o_(cathode)-E^o_(anode)$

Putting values in above equation, we get:

$E^o_(cell)=1.50-(0.0)=1.50V$

To calculate the EMF of the cell, we use the Nernst equation, which is:

$E_(cell)=E^o_(cell)-(0.059)/(n)\log ([H^(+)]^6)/([Au^(3+)]^2)$

where,

$E_(cell)$ = electrode potential of the cell = 1.23 V

$E^o_(cell)$ = standard electrode potential of the cell = +1.50 V

n = number of electrons exchanged = 6

$[H^(+)]=1.0M$

$[Au^(3+)]=?M$

Putting values in above equation, we get:

$1.23=1.50-(0.059)/(6)* \log(((1.0)^6)/([Au^(3+)]^2))$

$[Au^(3+)]=-1.0906* 10^(-6),1.096* 10^(-6)$

Neglecting the negative value because concentration cannot be negative.

Hence, the concentration of $Au^(3+)$ is $1.096* 10^(-6)$

Given the balanced equation representing a reaction:CH4(g) + 2O2(g) --> 2H2O(g) + CO2(g) + heat
Which statement is true about energy in this reaction?
(1) The reaction is exothermic because it releases heat.
(2) The reaction is exothermic because it absorbs heat.
(3) The reaction is endothermic because it releases heat.
(4) The reaction is endothermic because it absorbs heat.

Answers

The answer is (1) the reaction is exothermic because it releases heat. From the reaction, we can see that the heat is at the right of the equation which means the reaction releases heat. So it is called exothermic reaction. Endothermic reaction absorbs heat.

Answer: The answer is (2) the reaction is exothermic because it releases heat.

Which chemical equation represents the reaction of an Arrhenius acid and an Arrhenius base?(1) HC2H3O2(aq) + NaOH(aq) --> NaC2H3O2(aq) + H2O(l)
(2) C3H8(g) + 5 O2(g)--> 3 CO2(g) + 4 H2O(l)
(3) Zn(s) + 2 HCl(aq)--> ZnCl2(aq) + H2(g)
(4) BaCl2(aq) + Na2SO4(aq) --> BaSO4(s) + 2 NaCl(aq)

Answers

Answer : The correct option is, (1)

Explanation :

According to the Arrhenius acid-base concept,

Arrhenius acid is a species that produces $H^+$ ion in an aqueous solution and Arrhenius base is a species that produces $OH^-$ ion in an aqueous solution.

From the given options, option 1 chemical equation represents the reaction of an Arrhenius acid and an Arrhenius base. In this reaction, $HC_2H_3O_2$ produces $H^+$ ion in an aqueous solution and act as an Arrhenius acid, $NaOH$ produces $OH^-$ ion in an aqueous solution and act as an Arrhenius base.

While the other options does not represents the reaction of an Arrhenius acid and an Arrhenius base.

Reaction 2 is an example of combustion reaction.

Reaction 3 is an example of single-displacement reaction.

Reaction 4 is an example of double-displacement reaction.

Hence, the correct option is, (1)

The chemical equation that represents the reaction of an Arrhenius acid and an Arrhenius base is 1) HC2H3O2 (aq) + NaOH (aq) ---> NaC2H3O2 (aq) + H2O (I)

Which would most likely be the pH of a highly-corrosive acid

Answers

The answer is 1, (if it isn't, tell me the answer choices)

Answer:

a) 1

Explanation:

got it right 100%

Which type of organism helps return nutrients from dead plants and animals to the soil. A producer. B prey. C predator. D decomposer

Answers

The answer is D. Decomposer

The answer is 'decomposer.'

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