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3 years ago

Which of the following polyatomic ions has a 3- ionic charge?

Chemistry

1 answer:

ch4aika [34]3 years ago

4 0

Answer: Option (a) is the correct answer.

Explanation:

Poly means many and polyatomic ions means an ion(s) with two or more different atoms.

Out of the given options, phosphate ion is the polyatomic ion which has an ionic charge of 3-.

The formula depicting a phosphate ion is $PO_{4}^{3-}$ .

Whereas Nitrate, Sulfate, Hydroxide , Bicarbonate does not carry or have a 3- ionic charge.

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During the isothermal heat addition process of a Carnot cycle, 900 kJ of heat is added to the working fluid from a source at 400

Alinara [238K]

Answer:

the entropy change of the fluid during the process process is is 1.337 kJ/K, the change for the source is -1.337 kJ/K and the total entropy change is 0

Explanation:

since the Carnot cycle is a reversible cycle, the entropy change is related with the heat exchanged through:

ΔS =∫dQ/T

since the temperature remains constant

ΔS =∫dQ/T=(1/T)*∫dQ = Q/T

Q= heat added to the system

T= absolute temperature = 400°C= 673 K

therefore

ΔS = Q/T = 900 kJ/ 673 K = 1.337 kJ/K

ΔS working fluid = 1.337 kJ/K

since the process is reversible, the entropy change of the universe (total entropy change) is 0 (there is no entropy generation). thus

ΔS universe = ΔS working fluid + ΔS source = 0

ΔS source= -ΔS working fluid = -1.337 kJ/K

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3 years ago

Suppose the mole number of Ca2+ ions in a 50 mL water sample is quantified as 1.5 × 10−5 mol. What is the concentration of Ca2+

Anna11 [10]

$\frac{1.5x 10^{-5} mol Ca^{2+}}{50ml} ( \frac{1 mol CaC O_{3} }{1 mol Ca^{2+} } )( \frac{100,000 ppm}{1 molCaC O_{3}/L } ) \\ =0.0300234$

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3 years ago

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3 years ago

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What is the entropy change of the surroundings

KiRa [710]

Answer: The entropy change of the surroundings will be -17.7 J/K mol.

Explanation: The enthalpy of vapourization for 1 mole of acetone is 31.3 kJ/mol

Amount of Acetone given = 10.8 g

Number of moles is calculated by using the formula:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Molar mass of acetone = 58 g/mol

Number of moles = $\frac{10.8}{58}=0.1862moles$

If 1 mole of acetone has 32.3 kJ/mol of enthalpy, then

0.1862 moles will have = $\frac{32.3}{1}\times 0.1862=5.828kJ/mol$

To calculate the entropy change for the system, we use the formula:

$\Delta S_{sys}=\frac{\Delta H_{vap}}{T(\text{ in K)}}$

Temperature = 56.2°C = (273 + 56.2)K = 329.2K

Putting values in above equation, we get

$\Delta S_{sys}=\frac{5.828}{329.2}=0.0177kJ/Kmol=17.7J/Kmol$ (Conversion Factor: 1 kJ = 1000J)

At Boiling point, the liquid phase and gaseous phase of acetone are in equilibrium. Hence,

$\Delta S_{system}+\Delta S_{surrounding}=0$

$\Delta S_{surrouding}=-\Delta S_{system}=-17.7J/Kmol$

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3 years ago

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scoray [572]

The answer is 128.19

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