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Svetach [21]
3 years ago
12

A gas occupies a volume of 67.54 liters at 158°C and 4.87 atm pressure. Calculate the number of moles of this gas.

Chemistry
1 answer:
Katarina [22]3 years ago
6 0

Answer:

The number of moles of the gas is 9.295 moles or 9.30 moles

Explanation:

We use PV = nRT

Where P = 4.87 atm;

V = 67.54 L

R= 0.0821Latm/molK

T = 158 C = 158 +273 K = 431 K

the number of moles can be obtained by substituting the values in the respective columns and solve for n

n = PV / RT

n = 4.87 * 67.54 / 0.0821 * 431

n = 328.9198 / 35.3851

n = 9.295moles

The number of moles is approximately 9.30moles.

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A mixture of tea,<br> lemon juice, and<br> sugar is an example<br> of what?
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5 0
3 years ago
Calculate the value of E°cell for the following reaction:2Au(s) + 3Ca2+(aq) → 2Au3+(aq) + 3Ca(s)Au3+(aq) + 3e- → Au(s) E° = 1.50
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<u>Answer:</u> The standard electrode potential of the cell is -4.37 V

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For the given cell reaction:

2Au(s)+3Ca^{2+}(aq.)\rightarrow 2Au^{3+}(aq.)+3Ca(s)

The half reactions follows:

<u>Oxidation half reaction:</u>  Au(s)\rightarrow Au^{3+}(aq.)+3e^-;E^o_{Au^{3+}/Au}=1.50V     ( × 2 )

<u>Reduction half reaction:</u>  Ca^{2+}(aq.)+2e^-\rightarrow Ca(s);E^o_{Ca^{2+}/Ca}=-2.87V     ( × 3 )

Substance getting oxidized always act as anode and the one getting reduced always act as 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:

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8 0
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In photosynthesis, plants use energy from the sun to produce glucose, c6h12o6 , and oxygen from the reaction of carbon dioxide a
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Answer: 324 g (to 3 sf)

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Thus, the formula mass of carbon dioxide is:

6(15.9994)+12.011=108.0074 g/mol.

Thus, 3.00 mol has a mass of (108.0074)(3.00)=<u>324 g (to 3 sf)</u>

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