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Ksivusya [100]
2 years ago
8

1) How many grams of CO are needed to react with an excess of Fe2O3 to produce 209.7g Fe? Show your work.

Chemistry
2 answers:
klasskru [66]2 years ago
6 0
1.) is157.7 g
<span>moles Fe = 209.7 g/ 55.847 g/mol=3.75 
the ratio between Fe and CO is 2 : 3 
moles CO = 3.75 x 3 /2 =5.63 
mass CO = 5.63 mol x 28.01 g/mol=157.7 g

2.) is </span><span>1.06 moles 
</span>48.7/23 = 2.12 moles sodium 
<span>2.12/2 x 24 = 25.44dm^3 hydrogen = 1.06 moles </span>
1.06 X 6.02x10^23 = 1.204x10^24 molecules of hydrogen.

3.) is 91.8 
<span>8.3 moles H2S x (2 moles H2O / 2 moles H2S) = 8.3 moles H2O = theoretical amount produced. </span><span>8.3 moles H2O x (18.0 g H2O / 1 mole H2O) = 149 g H2O produced theoretically. </span><span>% yield = (actual amount produced / theoretical amount) x 100 = (137.1 g / 149 g) x 100 = 91.8 </span>
Travka [436]2 years ago
5 0
Mol Fe = 209.7/56 = 3.744 mol Fe
mol CO = 3.744 * 3/2 (mol ratio) = 5.616 mol CO
molecular weight of CO = 28
5.616 * 28 = 157.28 g CO needed

48.7/23 = 2.11 mol Na
2.11 * 1/2 = 1.055 mol H2
1.055 * 6.023*10^23 = 6.351 x 10^23 molecules of H2

8.3 * 2/2 = 8.3 mol H2O that could be produced
137.1/18 = 7.166 mol actually produced
7.616/8.3 * 100% = 91.75% produced (% yield)
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Answer:

Volume : 1.25 L

Explanation:

We are given here that the volume ( V_1 ) = 1.50 Liters, the initial moles ( held at 25 °C ) = 3.00 mol, and the final moles ( n_2 ) = 3.00 - 0.5 = 2.5 mol. The final mol is calculated given that 0.50 mol of gas are released from the prior 3.00 moles of gas.

Volume ( V_1 ) = 1.50 L,

Initial moles ( n_1 ) = 3.00 mol,

Final Volume ( n_2 ) = 3.00 - 0.5 = 2.5 mol

Applying the combined gas law, we can calculate the final volume ( V_2 ).

P_1V_1 / n_1T_1 = P_2V_2 / n_2T_2 - we know that the pressure and temperature are constant, and therefore we can apply the following formula,

V_1 / n_1 = V_2 / n_2 - isolate V_2,

V_2 = V_1 n_2 / n_1 = 1.50 L * 2.5 mol / 3.00 mol = ( 1.5 * 2.5 / 3 ) L = 1.25 L

The volume of the balloon will be 1.25 L.

6 0
3 years ago
A farmer selectively breeds tomatoes to be shipped to grocery stores across the United States. Which of the following genetic tr
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Answer:

D

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2 years ago
Which activity might help to increase the validity of this experiment?
MArishka [77]
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2 years ago
in the following reaction, how many grams of benzene (C6H6) will produce 42 grams of CO2? 2C6H6 + 15O2 → 12CO2 + 6H2O
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Answer: -

12.41 g

Explanation: -

Mass of CO₂ = 42 g

Molar mass of CO₂ = 12 x 1 + 16 x 2 = 44 g / mol

Number of moles of CO₂ = \frac{42}{44 g/mol}

= 0.9545 mol

The balanced chemical equation for this process is

2C₆H₆ + 15O₂ → 12CO₂ + 6H₂O

From the balanced chemical equation we see

12 mol of CO₂ is produced from 2 mol of C₆H₆

0.9545 mol of CO₂ is produced from \frac{2 mol C6H6 x 0.9545 mol  CO2}{12 mol CO2}

= 0.159 mol of C₆H₆

Molar mass of C₆H₆ = 12 x 6 + 1 x 6 =78 g /mol

Mass of C₆H₆ =Molar mass x Number of moles

= 78 g / mol x 0.159 mol

= 12.41 g

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