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

Question

4. [1pt]


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



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



a) A phase change is involved


b) Two moles of hydrogen gas react with two moles of oxygen gas to
produce two moles of water vapor


c) Energy is given off to the surroundings


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


e) ΔH for reacting one mole of hydrogen gas with a half mole of
of oxygen gas is −241.8 kJ





You must enter the letters you choose in one lower case group, with no spaces between.
Eg. if you choose a) d) and e) you would enter ade

Answer 1

b, c, and e. Those are all true.

Answer 2

a) False: Your reactants and products are both gases
b) False: Only one mole of Oxygen gas is need since oxygen gas is diatomic
c)True
d)False: Would be - 486.6 kj
e) False: Would be -243.3 kj

Answer 3

a) pretend: Your reactants and products are both gases b) pretend: in user-friendly words one mole of Oxygen gas is bypass with on the grounds that oxygen gas is diatomic c)authentic d)pretend: should be - 486.6 kj e) pretend: should be -243.3 kj

Answer 4

abc

Answer 5

B