When acetylene, C2H2, is burned in oxygen, carbon dioxide and steam are formed.

Question

When acetylene, C2H2, is burned in oxygen, carbon dioxide and steam are formed. A sample of acetylene with volume of 7.50L and a pressure of 1.00atm is burned in excess oxygen at 225°C. 2. Write a balanced equation for the reaction. How many moles of oxýgen are required to react with the acetylene? Ifair is 20% oxygen, what volume of air at STP is required? i. ii. iii. Note: STP is O°C and 1atm and acetylene is a gas .. The following is a multiple part question. A. For the following species provide the Lewis structures. List of species: water, sulfur trioxide, carbon dioxide, nitrite ion, methyl alcohol, hydrogen peroxide, methanal, methanoic acid, methylene chloride, and hydrogen bromide. B. From the list of species in part A list those species which are polar. C. Determination of formal charge. Follow the following instructions. Determine the formal charge of nitrogen in the nitrate ion, determine the formal charge of each oxygen in the nitrite ion, determine the formal charge of sulfur in sulfur dioxide. D. Bond angles: what is the O-S-O bond angle in sulfur dioxide, what is the O-C-O bond angle in carbon dioxide, what is the O-N-O bond angle in t nitrate ion, what is the H-O-H bond angle in hydrogen peroxide.

Explanation / Answer

Ans 2 :

i) The balanced reaction is given as :

2C2H2 + 5O2 = 4CO2 + 2H2O

ii) Using the ideal gas law , the number of moles of acetylene can be calculated

T = 225oC = 498.15 K

1.00 x 7.50 = n x 0.0821 x 498.15

n = 0.183 moles

So number of moles of oxygen gas required = (0.183 x 5) / 2

= 0.458 moles

iii)

since air is 20 % oxygen

Number of moles of air = (0.458 x 100) / 20 = 2.29 moles

The volume of air required will be : (2.29 x 0.0821 x 273.15) / 1.00

= 51.35 L

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