Question

1. Use information in the balanced chemical formula below to answer the next 4 questions

   C2H6                    +       7   F2             →           2 CF4             +         6 HF

mw = 30.06 amu                           mw = 37.99 amu                           mw = 88.00 amu               mw=20.00 amu         

a) How many moles of C2H6 would be consumed when reacted with 9.24 moles of F2?

b) If you consume 7.50 moles of F2, how many grams of HF are produced?

c) If 10.32 g of HF are generated, what mass of C2H6 was utilized as starting material?

d) What is the number of molecules of F2 required to completely consume 25.0 g of C2H6?

Answer 1

1. Use information in the balanced chemical formula below to answer the next 4 questions

   C2H6                    +       7   F2             →           2 CF4             +         6 HF

mw = 30.06 amu          mw = 37.99 amu        mw = 88.00 amu               mw=20.00 amu         

a) How many moles of C2H6 would be consumed when reacted with 9.24 moles of F2?

9.24 moles of F2 * 1 Mole of C2H6 / 7 mole of F2

= 1.32 Mole C2H6

b) If you consume 7.50 moles of F2, how many grams of HF are produced?

7.50 moles of F2 * 6 Mole HF / 7 mole F2

= 6.43 Mole HF

Amount of HF = number of moles * molar mass

= 6.43 Mole HF *20.00 g/ mole

= 128.6 g HF

c) If 10.32 g of HF are generated, what mass of C2H6 was utilized as starting material?

Mole of HF = 10.32 g/ 20.00 g / mole

= 0.516 moles

0.516 mole HF * 1 Mole C2H6/ 6 Mole HF

= 0.086 Mole C2H6

Amount of C2H6= 0.086 Mole C2H6 *30.06 g/ mole

= 2.56 g C2H6

d) What is the number of molecules of F2 required to completely consume 25.0 g of C2H6?

Number of mole of C2H6 =25.0 g of C2H6 /30.,06 g/mole

= 0.83 mole C2H6

0.83 mole C2H6 * 7 Mole F2 /1 mole C2H6

= 5.82 Mole F2

1 mol F2 = 6.023*10^23 molecules

5.82 Mole F2 *6.023*10^23 molecules /1 mol F2

= 3.51 *10^24 molecules