Introduction:
The behavior of a gas can be described using the ideal gas law, which assumes that the gas particles have no volume and do not interact with each other. However, in reality, gases deviate from ideal behavior under certain conditions. In this question, we are asked to determine the conditions under which a gas will exhibit ideal behavior.

Explanation:
To understand the conditions under which a gas will exhibit ideal behavior, let's consider the different options provided:

a) Low temperature and low pressure:
At low temperatures and low pressures, the gas particles have low kinetic energy and are far apart from each other. In this case, the intermolecular forces between the gas particles become significant, causing the gas to deviate from ideal behavior. Therefore, option 'a' is incorrect.

b) Low temperature and high pressure:
At low temperatures and high pressures, the gas particles are close together due to increased intermolecular forces. The volume occupied by the gas becomes significant compared to the volume of the container. As a result, the gas particles interact more strongly with each other, deviating from ideal behavior. Thus, option 'b' is also incorrect.

c) High temperature and low pressure:
At high temperatures and low pressures, the gas particles have high kinetic energy and are far apart from each other. The intermolecular forces between the gas particles are negligible, allowing the gas to behave ideally. As a result, option 'c' is correct.

d) High temperature and high pressure:
At high temperatures and high pressures, the gas particles are close together due to increased intermolecular forces. The volume occupied by the gas becomes significant compared to the volume of the container. As a result, the gas particles interact more strongly with each other, deviating from ideal behavior. Therefore, option 'd' is incorrect.

Conclusion:
In summary, a gas will exhibit ideal behavior at high temperatures and low pressures. At low temperatures and/or high pressures, the gas particles interact more strongly, deviating from ideal behavior. It is important to note that the ideal gas law is an approximation and does not perfectly describe the behavior of real gases under all conditions.