To find the number of grams of water, calculate the moles using the provided number of molecules and Avogadro's number. Then, multiply the moles by the molar mass of water (18.02 g/mol) to get approximately 113.53 grams of water.
To determine the number of grams of water in a container holding 3.8x1024 molecules of water (H2O) at STP (Standard Temperature and Pressure), we first need to calculate how many moles of water this represents.
One mole of any substance contains Avogadro's number of molecules, which is approximately 6.022x1023. Therefore, we can use this relationship to calculate moles:
Calculate the number of moles: Number of moles = (3.8x1024 molecules) ÷ (6.022x1023 molecules/mol).
This yields about 6.3 moles of water (since 3.8 ÷ 6.022 is approximately 6.3).
Next, using the molar mass of water, which is approximately 18.02 g/mol (2x1.008 g/mol for hydrogen and 15.999 g/mol for oxygen), we can convert moles to grams.
Multiply the moles by the molar mass: Mass in grams = 6.3 moles x 18.02 g/mol.
This calculation gives us approximately 113.53 grams of water in the container.
Therefore, there are approximately 113.53 grams of water inside the container at STP.