The Mass of Cyclopropane ($C_{3}H_{6}$) at STP
Cyclopropane ($C_{3}H_{6}$) is a highly flammable gas that is commonly used in various industrial applications. It is a three-membered ring hydrocarbon with each carbon atom bonded to two hydrogen atoms. In this article, we will explore the mass of cyclopropane when measured at STP (Standard Temperature and Pressure). To determine the mass of cyclopropane at STP, we need to consider its molar mass and the ideal gas law. The molar mass of cyclopropane can be calculated by summing the atomic masses of its constituent elements. Carbon has an atomic mass of approximately 12.01 g/mol, while hydrogen has an atomic mass of approximately 1.01 g/mol. Therefore, the molar mass of cyclopropane is: (3 * 12.01 g/mol) + (6 * 1.01 g/mol) = 42.09 g/mol Now, let's apply the ideal gas law, which states that the product of pressure, volume, and temperature is proportional to the number of moles of gas. At STP, the pressure is 1 atmosphere (atm) and the temperature is 273.15 Kelvin (K). The volume can be assumed to be 1 mole of cyclopropane gas. Using the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature, we can rearrange the equation to solve for the mass of cyclopropane. n = PV / RT Substituting the values for pressure, volume, and temperature, we get: n = (1 atm * 1 mol) / (0.0821 L * atm / mol * K * 273.15 K) Simplifying the equation, we find that the number of moles of cyclopropane is approximately 0.0409 mol. Finally, to calculate the mass of cyclopropane at STP, we multiply the number of moles by the molar mass: mass = 0.0409 mol * 42.09 g/mol The mass of cyclopropane at STP is approximately 1.72 grams. In conclusion, the mass of cyclopropane ($C_{3}H_{6}$) when measured at STP is approximately 1.72 grams. This calculation is based on the molar mass of cyclopropane and the application of the ideal gas law. It is important to note that this value may vary slightly depending on experimental conditions and the accuracy of measurements.