Chemistry question about a reaction and gas pressure...? Please help!!!

Posted on 2014-11-19 05:04:00 in Chemistry by TAYLOR

C2H5NO2 + 2H2O ? 2CO2 + NH3 + 3H2
You begin with 1.25 × 10-2 moles of glycine and an excess amount of water that will allow the reaction to proceed completely to products. This is all in a vessel with a volume of 850 mls at 27°C. Assume that the vessel begins with air at atmospheric pressure. Since glycine is a solid and water is a liquid, neglect any volume that they occupy as reactants. For all questions, assume that temperature remains constant unless told otherwise.

a. How many moles of gas are present at the start of the process (before any glycine has been consumed)?

b. What is the number of moles of gas produced if all of the glycine is consumed?

c. What is the final pressure of the system assuming that the volume remains constant?

d. If the vessel were allowed to expand keeping the pressure constant, what would the resulting volume be?

e. If the vessel can only expand to a volume of 1,250 ml, what is the resulting pressure?

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