I think this is a bad question, at least as you reproduced it here.
I can think of three situations that the question is really asking about. Based on how you interpret, either A, B, or C could be the answer. A would be the case in which you cool a gas down to a solid, and is the easiest to reason out. B is based on the fact that when gas is converted into solid, heat is released (exothermic) and that the temperature "in the flask" increases as a result. C is the case in which a gas turns to a solid at the deposition temperature. However, temperature of the substance does not change while the process is happening, so C makes sense. It all depends on what they mean by "temperature in the flask" and what they mean when a substance goes from gas to solid. Can you post the full question?
As far as some more things about heat and temperature though...
The reaction from gas to solid is not endothermic, but exothermic. The heat of deposition (or enthalpy*) is negative, and heat is released into the surroundings. It is wrong to say that heat decreases from state 1 to state 2. Certainly you have a negative value for heat, but that defines the direction of heat flow rather than a "decrease" in heat (negative = from system to surrounding). Heat is NOT a state function, and there is no such thing as Δq. Heat is characteristic of the process (chemical reaction, physical expansion, phase transition, etc.). You cannot say that at temperature 1, a substance has a certain heat value q1, and that at temperature 2, its heat value is q2.
What IS a state function is temperature. A functional definition of temperature is that it is an intensive (independent of amount (e.g. density)) physical property that drives heat flow between two systems. That is, if A is at a higher temperature than B, heat flows from A to B. It is related to "thermal energy" or "kinetic energy of random motion". Heat is defined as energy that flows between two systems at different temperatures. That seems like circular reasoning, so another definition for heat is that it is energy that drives random motion, rather than organized motion. Regardless, temperature of a system decreases when heat flows out of a system (q < 0), and increases when heat flows into a system (q > 0), generally. Hope you enjoy the wall of text.