# What is the total volume of the CO2(g) and H2O(g) produced by combustion of 1.00L of C2H6(g) at STP? [on hold]

I am very confused on how to solve this problem. I know that the balanced reaction is

$$\ce{2 C2H6 + 7 O2-> 4 CO2 + 6 H2O }$$

The temperature is 273.15 K and pressure is 1 atm but that's it.

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## put on hold as off-topic by Todd Minehardt, Tyberius, Karsten Theis, Jon Custer, MithoronJun 13 at 17:14

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• Welcome to chemistry SE. Can you show us the work you have already done? – Michael Lautman Jun 13 at 2:14
• Is the water in your equation a liquid or a gas? Are you familiar with the ideal gas law or maybe with Avogadro's law concerning amounts and volumes of gasses? – Karsten Theis Jun 13 at 3:25
• This is a nonsensical question where knowing some chemistry will get you into trouble. At STP most of the water would be a liquid, not a gas. However the problem specifically stipulates that you should consider the water produced as being in the gas phase. So assume all the product produced is in the gas phase. – MaxW Jun 13 at 4:33