What mass of lithium (in g) is required to react completely with 59.1 mL of gas at STP? given the equation 6Li+N2=2Li3

Your reaction equation should be

6Li + N2 = 2 Li3N

59.1 ml at STP is
(59.1*10^-3 l)/(22.4 l/mol)
= 2.64*10^-3 moles of N2.
That will react with 6 times as many moles of Li. Compute the mass of that.

To determine the mass of lithium required to react completely with nitrogen gas (N2) at STP (Standard Temperature and Pressure), we need to use the stoichiometry of the balanced equation.

From the given equation: 6Li + N2 → 2Li3N

We can see that 6 moles of lithium (Li) reacts with 1 mole of nitrogen gas (N2) to form 2 moles of lithium nitride (Li3N).

Step 1: Convert volume to moles of nitrogen gas
At STP, 22.4 L of any gas is equal to 1 mole. Therefore, 59.1 mL of nitrogen gas (N2) can be converted to moles using the following calculation:

59.1 mL × (1 L / 1000 mL) × (1 mole N2 / 22.4 L) = X moles of N2

Step 2: Calculate moles of lithium (Li) required
Since the stoichiometry of the balanced equation tells us that 6 moles of lithium react with 1 mole of nitrogen gas, we can write the following proportion:

6 moles Li / 1 mole N2 = X moles Li / (moles of N2 calculated in Step 1)

Step 3: Convert moles to grams
The molar mass of lithium (Li) is approximately 6.94 g/mol. Using this molar mass, we can calculate the mass of lithium required:

X moles Li × (6.94 g / 1 mole Li) = Mass of Li (in grams)

By following these steps, you can calculate the mass of lithium required to react completely with 59.1 mL of nitrogen gas at STP.

To solve this problem, we need to use stoichiometry, which is the calculation of the quantities of reactants and products in a chemical reaction.

Step 1: Write and balance the equation.

The given equation is: 6Li + N2 -> 2Li3N

Step 2: Determine the molar ratio.

From the balanced equation, we can see that 6 moles of Li react with 1 mole of N2 to produce 2 moles of Li3N. This gives us a molar ratio of 6:1:2 (Li:N2:Li3N).

Step 3: Convert the volume of gas to moles.

We are given the volume of gas at STP (standard temperature and pressure). At STP, one mole of any gas occupies 22.4 liters. We have 59.1 mL of gas, which is equivalent to 0.0591 liters. Thus, we can calculate the number of moles of N2 using the following formula:

moles of N2 = volume of gas (in liters) / 22.4

moles of N2 = 0.0591 L / 22.4 L/mol

Step 4: Calculate the moles of Li required.

Using the molar ratio from step 2, we know that for every 1 mole of N2, we need 6 moles of Li. Therefore, the moles of Li required can be calculated using the following formula:

moles of Li = moles of N2 * (6 moles Li / 1 mole N2)

Step 5: Convert moles of Li to grams.

Since we are asked for the mass of Li in grams, we need to convert the moles of Li to grams using its molar mass. The molar mass of Li is approximately 6.94 g/mol.

mass of Li (in grams) = moles of Li * molar mass of Li

Now, you can substitute the values from previous calculations into this formula to find the mass of Li required.