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Calculate the volume of a sample of carbon monoxide at 214°C and 367 torr if it occupies 3.65 L at 298 K and 745 torr.
My answer: 12.11 L (Please Check!)
My answer: 12.11 L (Please Check!)
To calculate the volume of carbon monoxide at a specific temperature and pressure, you can use the ideal gas law equation: V = (nRT)/P, where V is the volume of the gas, n is the number of moles of the gas, R is the ideal gas constant, T is the temperature in Kelvin, and P is the pressure in atmospheres. In this case, you will need to convert the given temperature of 214°C to Kelvin by adding 273 to it, giving you 487 K. Similarly, you will need to convert the pressure of 367 torr to atmospheres by dividing it by 760, giving you a pressure of 0.483 atm. Then, you can plug in these values into the equation and calculate the volume of carbon monoxide.
The ideal gas law is a mathematical equation that relates the pressure, volume, temperature, and number of moles of an ideal gas. It is used to calculate the volume of a gas when the other variables are known. The equation is V = (nRT)/P, where V is the volume, n is the number of moles, R is the ideal gas constant, T is the temperature in Kelvin, and P is the pressure in atmospheres. By rearranging the equation, you can solve for any of the variables as long as the others are known.
According to the ideal gas law, temperature and volume have a direct relationship. This means that as the temperature of a gas increases, its volume also increases proportionally, and vice versa. This can be explained by the kinetic theory of gases, which states that as temperature increases, the particles in a gas will move faster and take up more space, resulting in an increase in volume.
The unit for volume in the ideal gas law equation is typically expressed in liters (L) or cubic meters (m3). However, it can also be expressed in other units such as milliliters (mL) or cubic centimeters (cm3). It is important to make sure that all units are consistent when using the ideal gas law equation.
The ideal gas law is only applicable to ideal gases, which are theoretical gases that follow specific assumptions, such as having no intermolecular forces and occupying no volume. In reality, most gases do not behave like an ideal gas, especially at high pressures and low temperatures. Therefore, the ideal gas law can only be used as an approximation for real gases under certain conditions. For more accurate calculations, other gas laws such as the van der Waals equation can be used.