1a)Ethene (C2H4) burns in oxygen to give CO2 and H2O: C2H4 + 3 O2 --> 2 CO2 + 2

Question

1a)Ethene (C2H4) burns in oxygen to give CO2 and H2O: C2H4 + 3 O2 --> 2 CO2 + 2 H2O How many moles of oxygen are needed to react with 0.254 moles of ethene? ___ mols oxygen

1b) Study the chemical reaction below: C4H8 + 6 O2 4 CO2 + 4 H2O If 197 grams of O2 react, how many grams of water form? _____ g H2O

1c) You determine that the theoretical yield of a reaction is 50.0 g of product "X." You then go into the lab and run the experiment. You produce 25.0 g of product "X." What is your percent yield? ____ % yield

1d) How many mL of a 2.42 M NaOH solution is required to neutralize 37.6mL of 2.44M H2SO4?

H2SO4 (aq) + 2 NaOH (aq)   --->   2 H2O (l) + Na2SO4 (aq)

___ mL NaOH solution

1e) Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride:

S + 3 F2 ---> SF6

You place 3.5 g sulfur and 4.5 g fluorine in a reaction flask.

The maximum amount of SF6 that can be produced from the reaction is __________ g.

1f) How many grams of K2SO4 are in 250mL of 0.11 M K2SO4 solution?

___ g K2SO4

Explanation / Answer

1a)

C2H4 + 3 O2     ------------------> 2 CO2 + 2 H2O

1              3                                      2             2

0.254       ??

1 mol of ehene need ---------------- 3 mol of O2

0.254 mol ethene --------------->   ?? mol O2

moles of O2 = 0.254 x 3 / 1 = 0.762 moles

moles of O2= 0.762 moles

1b)

C4H8 + 6 O2 ------------------> 4 CO2 + 4 H2O

                192 g                                             72 g

                197 g                                              ??

mass of H2O = 197 x 72 / 192 = 73.88 g

mass of H2O= 73.88 g

1c)

percent yield = (actual yield / theoretical yield ) x 100

                        = (25 / 50 ) x 100

                        = 50%

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