Simple thermochemical equation

[SamTsui86]

1. Homework Statement
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 absorbed by the system, the reaction species

d) If the reaction takes place at constant volume, q and ΔH must by definition have the same value

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

Homework Equations

None

The Attempt at a Solution

I know that A is wrong because they are all gas.
I know that B is wrong because 2 mol of Hydrogen gas react with 1 mol of Oxygen gas
I know that C is wrong because energy was released
I think that D is right because that is no work
I think that E is also right

I've tried DE, E and D
but it's wrong, please help

 

[Bystander]

a) A phase change is involved
I know that A is wrong because they are all gas.

Check.

b) Two moles of hydrogen gas react with two moles of oxygen gas to
produce two moles of water vapor
I know that B is wrong because 2 mol of Hydrogen gas react with 1 mol of Oxygen gas

Check.

c) Energy is absorbed by the system, the reaction species
I know that C is wrong because energy was released

Check.

d) If the reaction takes place at constant volume, q and ΔH must by definition have the same value
I think that D is right because that is no work

Check.

e) ΔH for reacting four moles of hydrogen gas with two moles of
of oxygen gas is −483.6 kJ
I think that E is also right

"WORNG." Four plus two is twice the energy.

I've tried DE, E and D
but it's wrong, please help

If "D" is "wrong," it could be a matter of limited attempts allowed, or a mistranscription.