• What possible variables have you not accounted for? As you did the procedures, is it possible that the atmospheric pressure may have changed? If it did change over the course of your experiment, then how would your results have been affected?

During the seventeenth and especially eighteenth centuries, driven both by a desire to understand nature and a quest to make balloons in which they could fly (Figure 1), a number of scientists established the relationships between the macroscopic physical properties of gases, that is, pressure, volume, temperature, and amount of gas. Although their measurements were not precise by today’s standards, they were able to determine the mathematical relationships between pairs of these variables (e.g., pressure and temperature, pressure and volume) that hold for an ideal gas—a hypothetical construct that real gases approximate under certain conditions. Eventually, these individual laws were combined into a single equation—the ideal gas law—that relates gas quantities for gases and is quite accurate for low pressures and moderate temperatures. We will consider the key developments in individual relationships (for pedagogical reasons not quite in historical order), then put them together in the ideal gas law.

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with this one i know the answer in craters one reason i looked it up and i learned about it there is my evidence

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.