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balu736 [363]
4 years ago
6

SiO2(s) + 3C(s) --> SiC(s) + 2CO(g)

Chemistry
1 answer:
e-lub [12.9K]4 years ago
5 0
Since SiO2 is in excess the Carbon is the limiting reagent. In order to use stoichiometric ratios you must first convert to moles.

The molar mass of Carbon is 12 g/mol
13.4 g C * ( 1mol / 12 g) = 1.12 mol C

Now, for every 3 Carbon you get 2 Carbon monoxide.  
1.12 mol C * (2 CO / 3 C) = 0.74 mol CO

At Standard temperature and Pressure (STP); a mole of gas has a volume of 22.4 L. This is because everything in the Ideal Gas Law equation is held constant.

0.74 mol CO * ( 22.4 L/mol) = 16.7 L CO


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Answer:

The density is 0.0187 g/L

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First thing to do here is to calculate the Volume of 1 mole of CO2 using the ideal gas equation

Mathematically;

PV = nRT

thus V = nRT/P

what we have are;

n = 1 mole

R is the molar has constant = 0.082 L•atm•mol^-1•K^-1

P is the pressure = 0.0079 atm

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Substituting these values, we have;

V = nRT/P = (1 * 0.082 * 227)/0.0079

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This means according to the parameters given in the question, the volume of 1 mole of carbon iv oxide is 2,356.20 dm^3

But this is not what we want to calculate

What we want to calculate is the density

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density = molar mass/molar volume

Kindly recall that the molar mass of carbon iv oxide is 44 g/mol

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<h3>What is the molecular shape of a compound?</h3>

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Like here, the shape of nitrite is bent with lone pair which is shown by Lewis's structure The bond angle will be the distance between the nuclei of the neighbor atoms.

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brainly.com/question/7558603

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