6, ( 1 point) what is the mass % of carbon in each of the following compounds? a

Question

6, ( 1 point) what is the mass % of carbon in each of the following compounds? a. CHO 7. (1 point) Calculate how many moles of NO2 form when each quantity of reaction completely reacts. The balance equation is shown below. 2N,05 (g) 4NO2 (g) + 02 (g) a. 2.5 mol of NO b. 15.2 g of N,Os 8. (1 point) Calculate how many grams of N&Hs1;)is require when each quantity of product is fomed. The balance equation is shown below. (You will need to look up the molar masses) 2 N2H4 (1) 4 NHj (g) + N2 (g) a. 2.6 mol of NHs b. 3.44 gofN

Explanation / Answer

6)

a)CH2O

The formula mass of CH2O = 30 and mass due to carbon is 12

Thus mas % of Carbon in CH2O = mass of C x100/ formula mass

= 12 x100/30

= 40%

b) C6H12O6

Formula mass = 180 g/formula

and mass of Carbon = 72

Thus % mass of carbon = 72 x100/180

= 40%

7)

The balanced equation is

2N2O5 ----------> 4NO2 + O2

a) When 2 moles of N2O5 is used, 4 moles of NO2 are formed

Thus if 2.5 mol of N2O5 is used = 2.5x4/2 = 5 mol of NO2 s formed

b) mass of N2O5 used = 15.2 g

moles of N2O5 = mass / molar mass

= 15.2/108

= 0.1407 mol

thus moles of N2O5 formed = 0.1407 x4/2

= 0.2814 mol

8) the balanced equation is

2N2H4 -----------> 4NH3 + N2

a) 4 mole of Nh3 are fomed from 2 moles of N2H4

thus 26/17 mol of NH3 are fomed from = 26/17 x 2/4

=0.7647 mol of N2H4

mass of N2H4 required = moles x molar mass

= 0.7647 x 32g/mol

= 24.47 g of N2H4

b) 1 mole of N2 if ormed from 2 moles of N2H4

3.44/28 mol of N2 is formed from = (3.44/28)x2

= 0.2457 mol

thus mass of N2H4 needed = mol x molar mass

=0.2457molx 32g/mol

= 7.86 g

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