The Ideal Gas Law is PV = n R T, where "n" is the number of moles and "R = 8.314 J/mol.K" is the Universal Gas Constant. 1. Define P, V, and T in the equation above and give the unit for each term in the metric (SI) system. 2. Calculate the volume that a 0.3 mole sample of a gas will occupy at 270 K and a pressure of 2.0 atm. (1 atm. pressure = 1.01 x 10^5 N/m^2). 3. A sample of gas has a volume of 0.600 L at 300 K and a pressure of 0.8 atm. What is the number of moles in this sample? 4. What will happen to the volume of a gas under constant temperature if the pressure increases? (a) increase, (b) decrease, (c) explosion, (d) nothing. 5. As number of moles goes up, volume (a) goes down, (b) goes up, (c) stays the same.
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In the Ideal Gas Law, PV = nRT: - P represents pressure, and its unit in the SI system is Pascals (Pa). - V represents volume, and its unit in the SI system is cubic meters (m³). - T represents temperature, and its unit in the SI system is Kelvin (K). Show more…
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The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The ideal gas law is typically written as PV = nRT where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature. Rearrange the equation to solve for P. P = What is the pressure of 0.638 moles of an ideal gas at a temperature of 297.0 K and a volume of 5.58 L? P = atm
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The Ideal Gas Law states that $P V=n R T$ where $P$ is pressure, $V$ is volume, $n$ is the number of moles of gas, $R$ is a fixed constant (the gas constant), and $T$ is absolute temperature. Show that $\frac{\partial T}{\partial P} \cdot \frac{\partial P}{\partial V} \cdot \frac{\partial V}{\partial T}=-1$
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