sample of noble gas was collected at STP. If 0.0500 g of the gas occupies 0.0284 dm3, determine the identity of the gas.The gas has a molar mass of  g mol−1. This gas is identified as .Give your answer to 3 significant figures and answer with the name or symbol for the gas.

The question seems to be incomplete as the molar mass of the gas is not provided. However, I can guide you on how to solve this problem once you have the molar mass.

1. First, you need to convert the mass of the gas from grams to moles. This can be done using the molar mass of the gas. The formula to use is: moles = mass (g) / molar mass (g/mol).

2. Next, you need to find the volume of one mole of the gas at STP (Standard Temperature and Pressure). According to Avogadro's law, one mole of any gas at STP occupies 22.4 dm3.

3. Then, you need to find the volume that the number of moles you calculated in step 1 would occupy at STP. This can be done by multiplying the number of moles by 22.4 dm3.

4. Finally, compare the volume you calculated in step 3 with the volume given in the problem (0.0284 dm3). If they match, then the gas you have is the one whose molar mass you used in step 1.

Without the molar mass, it's impossible to identify the gas. Please provide the molar mass so I can help you identify the gas.