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 not involved
b) Two moles of hydrogen gas react with one mole 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 four moles of hydrogen gas with two moles of
of oxygen gas is −483.6 kJ
2007-01-27 13:06:56 · 7 answers · asked by Whatever 1 in Science & Mathematics ➔ Chemistry
abd
2007-01-27 13:21:16 · answer #1 · answered by mazo 1 · 0⤊ 0⤋
See the hints I gave to another of your classmates who sent in the same question around 7:45pm.
Why don't you guys work together????
2007-01-27 14:59:42 · answer #2 · answered by teachbio 5 · 0⤊ 0⤋
actually the chemical reactions are below not above. sorry about that, but your question is faulty.
2007-01-27 13:10:49 · answer #3 · answered by UpNorthDownSouth 2 · 0⤊ 0⤋
i beleive its 2h20=h2o-11 ++24+h20
2007-01-27 18:55:43 · answer #4 · answered by deanrusk44 1 · 0⤊ 0⤋
a) fake: Your reactants and products are both gases b) fake: only one mole of Oxygen gas is go with in view that oxygen gas is diatomic c)authentic d)fake: must be - 486.6 kj e) fake: must be -243.3 kj
2016-10-16 04:57:47 · answer #5 · answered by curella 4 · 0⤊ 0⤋
d
2007-01-27 13:10:39 · answer #6 · answered by Anonymous · 0⤊ 0⤋
a-true
b-true
d- true
these are true for sure
2007-01-28 09:59:28 · answer #7 · answered by lenny b 1 · 0⤊ 0⤋