Hello!!! I need help solving this. Consider this combustion reaction. C6H12O6(s)

Question

Hello!!! I need help solving this.
Consider this combustion reaction. C6H12O6(s)+6O2(g)=6CO2(g)+6H2O(l) A) What is partial pressure of CO2 if 0.0234 moles are produced at a 23.4'C in a sealed 500.0ml flask?
I know that partial pressure would be P=NRT/V but I'm confused because they gave me the moles and the reaction. There is 6 CO2 what do I do with the 6? Can someone show me how to find the partial pressure please.
B) Based on information above what would be the new pressure if the sample were transferred to a smaller 150.00ml flask and cooled to -10.5'C?
Thank you!

Hello!!! I need help solving this.
Consider this combustion reaction. C6H12O6(s)+6O2(g)=6CO2(g)+6H2O(l) A) What is partial pressure of CO2 if 0.0234 moles are produced at a 23.4'C in a sealed 500.0ml flask?
I know that partial pressure would be P=NRT/V but I'm confused because they gave me the moles and the reaction. There is 6 CO2 what do I do with the 6? Can someone show me how to find the partial pressure please.
B) Based on information above what would be the new pressure if the sample were transferred to a smaller 150.00ml flask and cooled to -10.5'C?
Thank you!


Consider this combustion reaction. C6H12O6(s)+6O2(g)=6CO2(g)+6H2O(l) A) What is partial pressure of CO2 if 0.0234 moles are produced at a 23.4'C in a sealed 500.0ml flask?
I know that partial pressure would be P=NRT/V but I'm confused because they gave me the moles and the reaction. There is 6 CO2 what do I do with the 6? Can someone show me how to find the partial pressure please.
B) Based on information above what would be the new pressure if the sample were transferred to a smaller 150.00ml flask and cooled to -10.5'C?
Thank you!

Explanation / Answer

ideal gas equation

PV = nRT

A)

volume = 500 ml = 500*10^-6 m^3

P = 0.0234*8.314*(273 + 23.4)/(500*10^-6) = 115327.81 Pa

B)

P = 0.0234*8.314*(273 - 10.5)/(150*10^-6) = 340458.3 Pa

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