1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid dodecane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.22 kg of dodecane are burned in air at a pressure of exactly and a temperature of 17.0°C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to significant digits.

2.  369 L

Explanation:

1. Combustion is a chemical reaction in which hydrocarbons are burnt in the presence of oxygen to give carbon dioxide and water.

The balanced chemical reaction is:

2. To calculate the moles, we use the equation:

According to stoichiometry :

2 mole of dodecane produces = 24 moles of carbon dioxide

Thus 1.29 moles of dodecane produces = of carbon dioxide

According to ideal gas equation:

P = pressure of gas = 1 atm

V = Volume of gas = ?

n = number of moles = 15.5

R = gas constant =

T =temperature =

Thus the volume of carbon dioxide gas that is produced is 369 L

the answer is 0.42 is that is an option. this question provides no info