[Stella26]

I've been unable to find the answer to this question. I'd be grateful if any of you could help. Thanks in advance! Here is the question:

Consider the combustion of sucrose (C₁₁H₂₂0₁₁), sucrose and oxygen gas combine to form liquid water and a gaseous carbon dioxide.
        a. Write and balance the equation, including phases.
        b. If 2,001g sucrose reacts with 1.00L of O² at 753 torr and 25.8°C, how many grams of liquid water are theoretically formed?
        c. If the volume of the reaction vessel stays fixed, but the temperature increases by 3.27°C during the reaction, what pressure of gaseous product is formed?

*{MOD Edit -- improve title}*

[Hunter2]

Please sow first your attempt. We dont solve homework here. So tell what is unclear.

a) To develop the reaction equation should be easy. write left the sugar and right the water and carbon dioxide. Add the coefficients.
b) convert the values of the the physical parameter into SI-units. Use ideale gas equation to get the mole and mass of oxygen of 1 l. compare this to mass which 2,01g copper needs according the reaction eaquation. If you have this numbers you can also calulate the amount of water.
c.) How many mole in the vessel convert condition to new temperature.