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3 years ago

2) A sample of table sugar (sucrose C12H22O11) has a mass of 1.202g

Chemistry

1 answer:

Basile [38]3 years ago

6 0

Answer:

A) 0.003512 moles

Carbon = 0.04214 moles

Hydrogen = 0.07726 moles

Oxygen = 0.03863 moles

C) Carbon = 2.54*10^22 atoms

Hydrogen = 4.65 *10^22 atoms

Oxygen = 2.33 * 10^22 atoms

Explanation:

Step1: Data given

Mass of sucrose = 1.202 grams

Molar mass of sucrose = 342.3 g/mol

Step 2: Calculate moles of sucrose

Moles sucrose = mass / molar mass

Moles sucrose = 1.202 grams / 342.3 g/mol

Moles sucrose = 0.003512 moles

Step 3: Calculate the moles of each element in C12H22O11.

For 1 mol of sucrose we have 12 mol of carbon, 22 mol of hydrogen and 11 mol of oxygen

Carbon = 12*0.003512 = 0.04214 moles

Hydrogen = 22* 0.003512 = 0.07726 moles

Oxygen = 11* 0.003512 = 0.03863 moles

Step 4: Calculate the number of atoms of each type in C12H22O11.

Carbon = 0.04214 moles * 6.022*10^23/mol = 2.54*10^22 atoms

Hydrogen = 0.07726 moles * 6.022*10^23/mol = 4.65 *10^22 atoms

Oxygen = 0.03863 moles * 6.022*10^23/mol = 2.33 * 10^22 atoms

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The mass of an average blueberry is 0.75 g and the of am automoblie is 2.0 x 10 to the 3 Kg. Find the number of automobiles whos

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Answer : The number of automobiles needed are, $2.26\times 10^{17}$

Explanation :

First we have to calculate the mass of blueberries.

As, 1.0 mole of blueberries contains $6.022\times 10^{23}$ blueberries

So, 0.75 grams of blueberries contains $0.75g\times 6.022\times 10^{23}=4.52\times 10^{23}g$ blueberries

Mass of blueberries = $4.52\times 10^{23}g$

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Number of automobiles needed = $\frac{4.52\times 10^{23}g}{2.0\times 10^{3}kg}$

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3 years ago

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3 years ago

When 5.58g H2 react by the following balanced equation, 32.8g H2O are formed. What is the percent yield of the reaction? 2H2(g)+

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Answer:

D) 65.7%

Explanation:

Based on the reaction:

2H2(g)+O2(g)⟶2H2O(l)

<em>2 moles of hydrogen produce 2 moles of water assuming an excess of oxygen.</em>

<em />

To find percent yield of the reaction we need to find theoretical yield (The yield assuming all hydrogen reacts producing water). With theoretical yield and actual yield (32.8g H₂O) we can determine percent yield as 100 times the ratio between actual yield and theoretical yield.

<em>Theoretical yield:</em>

Moles of 5.58g H₂:

5.58g H₂ ₓ (1 mol / 2.016g) = 2.768 moles H₂

As 2 moles of H₂ produce 2 moles of H₂O, if all hydrogen reacts will produce 2.768 moles H₂O. In grams:

2.768 moles H₂O ₓ (18.015g / mol) =

49.86g H₂O is theoretical yield

<em>Percent yield:</em>

Percent yield = Actual yield / Theoretical yield ₓ 100

32.8g H₂O / 49.86g ₓ 100 =

65.7% is percent yield of the reaction

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4 years ago