Consider 1.00 mole samples of N_2O_4 and N_2H_4. Which of the following statemen

Question

Consider 1.00 mole samples of N_2O_4 and N_2H_4. Which of the following statements regarding these two samples is FALSE? Both of the samples have the same mass. Both of the samples have the same number of atoms. Both of the samples have the same number of molecules. Both of the samples are nonelectrolytes. More than one of the statements above is false. Which of the following statements regarding this reaction is FALSE? The moles of C_2H_6O and CO_2 produced in this reaction will be equal to one another. 1 molecule of C_6H_12O_4 can produce 2 molecules of C_2H_4O and 2 molecules of CO_2. 4.5 moles of C_6H_12O_6 can produce 9 moles of C_2H_6O. 100 g of C_6H_12O_6 would produce a sum total of 100 g C_2H_6O and CO_6. 1 g of C_6H_12O_6 can produce 2 g C_2H_6O and 2 g CO_2. A student carries out the reaction shown question 7 using 2.500 moles of C_6 H_12O_6. The student actually obtains 100.0 g of C_2H_6O as a result of the reaction. What is the student's percent yiel

Explanation / Answer

(6)

Molar mass of N2O4 is 92 g/mol

Molar mass of N2H4 is 32 g/mol

So, mass of each mole are not same.

(7)

For a chemical balanced reaction always moles ratio will be same.

Means you can divide with any number on both sides.

1 mol of C6H12O6 gives 2 moles of C2H6O and 2 moles of CO2

Similarly with molecules also.

As i told you chemical reaction depends on moles but not mass.

So, 1 g mass of C6H12O6 willnot give 2 g mass of C2H6O

here you should convert them into moles by dividing with molar mass.

so, 1 g C6H12O6 means = 1/180 = 0.0055 moles

So we get 2 x 0.0055 moles of C2H6O

Now convert into mass, Molar mass of C2H6O = 46 g/mol

0.0055 x 46 =0.255 g

which is not equal to 2.

So , false statement is (D)

(8)

So from reaction, 2.5 moles of C6H12O6 gives 2x 2.5 moles of C2H6O = 5 moles

5 moles of C2H6O weighs = 5 x 46 = 230 g

percentage yield = actual mass /theoritical x 100 = 100/230 x 100 == 43.41%

(9)

we will do elemental analysis here

CO2 moles is 3.687 moles .this means in CO2 we have 1 carbon, so reactant contains 3.687 moles of Carbon

In H2O we have 2 hydrogens, so total hydrogen moles = 2 x 1.844 moles == 3.688 moles

Moles ratio of C:H = 3.687 : 3.688 = 1:1

So, empirical formula = CH

Given molar mass = 72 g/mol

we know molecular formula = n(CH)

To get n = molar mass / mass of emperical formula = 72 / (13) = 6

So, moleuclar formula = 6 x (CH) = C6H6

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