Which of the following are true statements for the above chemical reaction ?

Question

2H2(g) + O2(g) --> 2H2O(g) ΔH = −486.6kJ

a) A phase change is involved


b) Two moles of hydrogen gas react with one mole of oxygen gas to
produce two moles of liquid water


c) Energy is absorbed by the system, the reaction species


d) If the reaction takes place at constant pressure, q = −483.6 kJ


e) ΔH for reacting four moles of hydrogen gas with two moles of
of oxygen gas is −483.6 kJ

Answer 1

You and medstudent and geebeegeebee should get together and try to figure this one out. Thrre brains are better than one, if you are all serious about learning.

What you need to know:
a) what is a phase change, and how would this be described in a reaction formula?
b) how do you know how to read a reaction formula, ie. what are the mole ratios?
c) How is energy absorbtion or release shown in a reaction formula, ie. is delta H positive or negative?
d) what does pressure have to do with a reaction?
e) how can the info from one reaction be used to predict about a related reaction.

Chem-is TRY!!!! Best of luck, as chem gets much harder than this.

Answer 2

a) pretend: Your reactants and products are the two gases b) pretend: basically one mole of Oxygen gas is circulate with considering that oxygen gas is diatomic c)authentic d)pretend: could be - 486.6 kj e) pretend: could be -243.3 kj