Please show me the steps.....
At STP, 3.00 L of nitrogen gas contains the same number of molecules as
A) 1.00 L of nitrogen gas
B) 2.00 L of oxygen gas
C) 3.00 L of chlorine gas
D) 4.00 L of hydrogen gas
Give me that damn answer.
How many moles are present in 30.0 L of helium gas at STP?
To determine which option contains the same number of molecules as 3.00 L of nitrogen gas at STP (Standard Temperature and Pressure), we need to use the concept of Avogadro's Law.
According to Avogadro's Law, equal volumes of gases at the same temperature and pressure contain an equal number of molecules.
So, let's compare the given options:
A) 1.00 L of nitrogen gas: Since 3.00 L of nitrogen gas is given to be the reference, this option contains a smaller volume of nitrogen gas. Therefore, it cannot contain the same number of molecules.
B) 2.00 L of oxygen gas: Again, this option contains a smaller volume of gas compared to 3.00 L of nitrogen gas. So, it cannot contain the same number of molecules.
C) 3.00 L of chlorine gas: This option has the same volume as the given reference. Since equal volumes contain an equal number of molecules, this could potentially be the correct option.
D) 4.00 L of hydrogen gas: This option contains a larger volume of gas compared to 3.00 L of nitrogen gas. Hence, it cannot contain the same number of molecules.
Therefore, the correct answer is C) 3.00 L of chlorine gas, as it has the same volume as the given reference of nitrogen gas at STP and thus contains the same number of molecules.
You don't need an steps. Avogadro's Law says that equal volume of (ideal) gases at the same temperature and pressure contain the same number of molecules. So you had 3.00 L of one gas, you look for the answer of 3.00 L of another gas if you are looking for the same number of molecules.
You MAY calculate if you wish, using the ideal gas law equation.
PV = nRT
For the same P, V, and T, n will be the same for any gas; therefore, the number of molecules will be the same.