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3 years ago

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What is the total mass (amu) of carbon in each of the following molecules?

1 answer:

Rama09 [41]3 years ago

4 0

Answer:

The atomic mass of carbon (C) is 12.0107 amu, so if you want to calculate the total mass in each molecule, you just need to multiply the number of carbon atoms in the substance by 12.017. In (a) there is one atom of C, (b) have also one atom of C, (c) have 12 atoms of C, and (d) have five atoms of C. Thus, the total mass (amu) of carbon is:

(a) 12.017 amu

(b) 12.017 amu

(c) 144.204 amu

(d) 60.085 amu

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Which substance has a giant covalent structure and contains atoms of more than one element?A diamondB graphiteC methaneD sand

marysya [2.9K]

which substance has a giant covalent structure and contains atoms of more than one elements?

Explanation:

answer:methane

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3 years ago

The magnesium atom in chlorophyll A. is used to pass excited electrons on to pheophytin B. is coupled to the production of ATP C

goblinko [34]

Answer:

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Explanation:

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4 years ago

Calculate the number of moles in the following: 2.8 X 10^24 atoms of Cl2

vova2212 [387]

Answer:

<h3>The answer is 4.65 moles</h3>

Explanation:

To find the number of moles given it's number of entities we use the formula

$n = \frac{N}{L} \\$

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question

N = 2.8 × 10²⁴ atoms of Cl2

So we have

$n = \frac{2.8 \times {10}^{24} }{6.02 \times {10}^{23} } \\ = 4.65116279069...$

We have the final answer as

<h3>4.65 moles</h3>

Hope this helps you

7 0

3 years ago

A galvanic cell at a temperature of 42 degrees Celcius is powered by the following redox reaction:

seropon [69]

<u>Answer:</u> The cell voltage of the given reaction is 1.86 V

<u>Explanation:</u>

The given chemical equation follows:

$3Cu^{2+}(aq.)+2Al\rightarrow 2Al^{3+}(aq.)+2Au(s)$

<u>Oxidation half reaction:</u> $Al(aq.)\rightarrow Al^{3+}(aq.)+3e^-;E^o_{Al^{3+}/Al}=1.66V$ ( × 2)

<u>Reduction half reaction:</u> $Cu^{2+}(aq.)+2e^-\rightarrow Cu(s);E^o_{Cu^{2+}/Cu}=0.16V$ ( × 3)

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:

$E^o_{cell}=0.16-(-1.66)=1.82V$

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

$E_{cell}=E^o_{cell}-\frac{2.303RT}{nF}\log \frac{[Al^{3+}]^2}{[Cu^{2+}]^3}$

where,

$E_{cell}$ = electrode potential of the cell = ? V

$E^o_{cell}$ = standard electrode potential of the cell = +1.82 V

n = number of electrons exchanged = 2

R = Gas constant = 8.314 J/mol Kl

T = temperature = $42^oC=[42+273]K=315K$

F = Faraday's constant = 96500

$[Al^{3+}]=1.63M$

$[Cu^{2+}]=3.43M$

Putting values in above equation, we get:

$E_{cell}=1.82-\frac{2.303\times 8.314\times 315}{2\times 96500}\times \log(\frac{(1.63)^2}{(3.43)^3})\\\\E_{cell}=1.86V$

Hence, the cell voltage of the given reaction is 1.86 V

4 0

3 years ago

What is the percent nitrogen in each of the following compounds?

Zinaida [17]

Answer:

N 2 H4

Explanation:

7 0

3 years ago

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