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3 years ago

4. The mass of a silver liberty (coin) was measured three times and each measurement was made

Chemistry

1 answer:

Vaselesa [24]3 years ago

7 0

Answer:

The average mass of the gold coin reported to five significant figures, even though you had to divide by "3" to obtain the average.

Explanation:

Given that,

The mass of a silver liberty was measured three times and each measurement was made to five digits.

The mass values are,

$m_{1}=12.519\ g$

$m_{2}=12.521\ g$

$m_{3}=12.496\ g$

The average mass of the gold coin is 12.512 g.

We know that,

Significant figures :

Significant figures is explained the nonzero, leading zero and zeros between two nonzero digits.

For example,

The digits is 0.003405

In the digit, 345 = nonzero

0.00 = leading zero

The average mass of the gold coin reported to five significant figures because average mass is 12,512. All digits are nonzero.

Nonzero digit are significant.

Hence, The average mass of the gold coin reported to five significant figures, even though you had to divide by "3" to obtain the average.

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Answer:

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Explanation:

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Hydrogen ions cannot exist alone but they exist after combining with water molecules true or false

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How many molecules are in 4.00 x 10^2mg of ibuprofen?

Serggg [28]

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How to solve for K when given your anode and cathode equations and voltage

Aleks04 [339]

Answer:

See Explanation

Explanation:

In thermodynamics theory the Free Energy (ΔG) of a chemical system is described by the expression ΔG = ΔG° + RTlnQ. When chemical system is at equilibrium ΔG = 0. Substituting into the system expression gives ...

0 = ΔG° + RTlnKc, which rearranges to ΔG° = - RTlnKc. ΔG° in electrochemical terms gives ΔG° = - nFE°, where n = charge transfer, F = Faraday Constant = 96,500 amp·sec and E° = Standard Reduction Potential of the electrochemical system of interest.

Substituting into the ΔG° expression above gives

-nFE°(cell) = -RTlnKc => E°(cell) = (-RT/-nF)lnKc = (2.303·R·T/n·F)logKc

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Application example:

Calculate the Kc value for a Zinc/Copper electrochemical cell.

Zn° => Zn⁺² + 2e⁻ ; E°(Zn) = -0.76 volt

Cu° => Cu⁺² + 2e⁻ ; E°(Cu) = 0.34 volt

By natural process, charge transfer occurs from the more negative reduction potential to the more positive reduction potential.

That is,

Zn° => Zn⁺² + 2e⁻ (Oxidation Rxn)

Cu⁺² + 2e⁻ => Cu° (Reduction Rxn)

E°(Zn/Cu) = (0.0592/n)logKc

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=> logKc = 2(1.10)/0.0592 = 37.2

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