Oblivion77 said:I was thinking PV=nRT but it might not be.
Nothing really
Borek said:That's the right one, although not sufficient one.
Get back once you try.
Oblivion77 said:Do I need to use the fact that 1mol = 22.4L at STP?
STP stands for Standard Temperature and Pressure, which is a standardized set of conditions used to measure gases. It is defined as 0°C (273.15 K) and 1 atmosphere (atm) pressure.
To identify a gas at STP, you need to know its volume and mass. Once you have these values, you can use the ideal gas law (PV = nRT) to calculate the number of moles (n) of the gas. Then, you can use the molar mass of the gas to determine its identity.
The ideal gas law is a mathematical equation that describes the behavior of ideal gases. It states that the pressure (P), volume (V), number of moles (n), and temperature (T) of a gas are all related by the equation PV = nRT, where R is the gas constant.
To calculate the molar mass of a gas, you first need to know its volume, mass, and number of moles. Using the ideal gas law, you can calculate the number of moles (n) of the gas. Then, you can divide the mass of the gas by the number of moles to get the molar mass.
To determine the gas in this question, we first need to calculate the number of moles of the gas. Using the ideal gas law, we get n = PV/RT = (1 atm * 2.75 L)/(0.0821 L*atm/mol*K * 273.15 K) = 0.105 mol. Then, we can divide the mass of the gas (5.39 g) by the number of moles (0.105 mol) to get the molar mass of the gas, which is approximately 51.3 g/mol. Based on this value, we can determine that the gas is likely sulfur hexafluoride (SF6).