Does hydrogen react with air at room temperature and pressure?
According to the Encyclopedia Britannica, to somewhat paraphrase this non-technical source, the reaction rate of $\ce{O2(g)}$ and $\ce{H2(g)}$ at atmospheric pressure is not measurable at any mixing ratio at temperatures below $\ce{300^oC}$.  Unfortunately that source does not report what kind of experimental detection limits define what &quot;not measurable&quot; means.
These class notes from the University of Toronto Institute for Aerospace Studies, AER1304 course state this in more dramatic fashion:

The reaction between hydrogen and oxygen is a good example of a
multicomponent kinetic system. To describe the system properly, we
should consider eight major species and at least 16 reactions.
[The overall] reaction is exothermic, but mixtures of gaseous hydrogen and oxygen are quite stable at
atmospheric conditions. Any conceivable direct reaction between the
two gases is zero.

The reaction half-time at atmospheric [pressures] has been estimated to be much larger than the age of the universe.
If the reaction is initiated by some free-radical species, then the reaction proceeds very rapidly and violently.


So the manner in which the reaction rate of $\ce{O2(g)}$ with $\ce{H2(g)}$ increases with temperature is very complex, though basically negligible in the absence of a catalyst until you reach the auto-ignition temperature.
According to this Wikipedia article:

The hydrogen autoignition temperature, the temperature of spontaneous
ignition in air, is 500 °C.

Notice that this says air not oxygen. The $\ce{H2}$ concentrations for the basis of this statement range from 4% to 74%.  This seems like quite a large range to give a single result for autoignition temperature, but given the great complexities of the $\ce{H2}$ + $\ce{O2}$ reaction, some estimations are clearly necessary in order to discuss this question in a reasonably concise fashion.
One note about the question regarding the composition and contents of the container; I'd be sure that it never contained any high surface-area platinum powder or be coated with any sort of perchlorate residues or any such ridicules thing!  The whole issue with the difficulty in getting this highly exothermic reaction to proceed is kinetics.  As eluded to in some of the comments, there are chemical catalysts that can help the reaction get over this large energy barrier, it doesn't have to be a spark!