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2 years ago

4. Calculate the empirical formula for the following compounds Na=32.4% S=22.6 % O=45.0%

Chemistry

1 answer:

lilavasa [31]2 years ago

7 0

Answer:

Na2 S O4

Explanation:

Na mole wt 22.989

32.4 / 22.989 = 1.4093

S mole wt = 32.06

22.6/32.06 = .7049

O mole wt = 15.999

45 / 15.999 = 2.8127 Now divide all of the results by the smallest

Na 1.4093 / .7049 = 2

S .7049/.7049 = 1

O 2.8127 /.7049 = 4 so Na2 S O4

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3 years ago

What mass, in grams, of CO2 and H20 N is formed from 2.55 mol of propane?

Black_prince [1.1K]

Answer: The mass of $CO_2$ and $H_2O$ produced are 336.6 g and 183.6 g respectively.

Explanation:

The combustion reaction between propane and oxygen leads to formation of carbon dioxide and water.

Law of Conservation of mass states that the mass will remain constant for a balanced equation. This is carried out when the total number of atoms on reactant side is same as the total number of atoms on the product side. Thus the equation must be balanced.

$C_3H_8+5O_2\rightarrow 3CO_2+4H_2O$

a) 1 mol of propane produces = 3 moles of $CO_2$

Thus 2.55 mol of propane produces = $\frac{3}{1}\times 2.55=7.65 moles of [tex]CO_2$

mass of $CO_2=moles\times {\text {molar mass}}=7.65mol\times 44g/mol=336.6g$

b) 1 mol of propane produces = 4 moles of $H_2O$

Thus 2.55 mol of propane produces = $\frac{4}{1}\times 2.55=10.2 moles of [tex]H_2O$

mass of $H_2O=moles\times {\text {molar mass}}=10.2mol\times 18g/mol=183.6g$

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3 years ago

Consider the following balanced equation. SiO2(s)+3C(s)→SiC(s)+2CO(g) Complete the following table, showing the appropriate numb

vlada-n [284]

Answer:

mol(SiO₂) mol(C) mol(SiC) mol(CO)

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2.5 7.5 2.5 5.0

1.4 4.2 1.4 2.8

Explanation:

From the balanced equation:

SiO₂(s) + 3C(s) → SiC(s) + 2CO(g),

It is clear that 1.0 mole of SiO₂ reacts with 3.0 moles of C to produce 1.0 mole of SiC and 2.0 moles of CO.

We can complete the table of no. of moles of each component:

1. 9.0 moles of C:

We use the triple amount of C, so we multiply the others by 3.0.

So, it will be 3.0 moles of SiO₂ with 9.0 moles of C that produce 3.0 moles of SiC and 6.0 moles of CO.

2. 1.0 mole of SiO₂:

We use the same amount of SiO₂ as in the balnced equation, so the no. of moles of other components will be the same as in the balanced equation.

So, it will be 1.0 moles of SiO₂ with 3.0 moles of C that produce 1.0 moles of SiC and 2.0 moles of CO.

3. 26.0 moles of CO:

We use the amount of CO higher by 13 times than that in the balanced equation, so we multiply the others by 13.0.

So, it will be 13.0 moles of SiO₂ with 39.0 moles of C that produce 13.0 moles of SiC and 26.0 moles of CO.

4. 7.5 moles of C:

We use the amount of C higher by 2.5 times than that in the balanced equation, so we multiply the others by 2.5.

So, it will be 2.5 moles of SiO₂ with 7.5 moles of C that produce 2.5 moles of SiC and 5.0 moles of CO.

5. 1.4 moles of SiO₂:

We use the amount of SiO₂ higher by 1.4 times than that in the balanced equation, so we multiply the others by 1.4.

So, it will be 1.4 moles of SiO₂ with 4.2 moles of C that produce 1.4 moles of SiC and 2.8 moles of CO.

5 0

3 years ago