2NaN3(s)==>2Na(s) + 3N2(g)
How many liters of N2 are produced at STP if the air bag contains 114g of NaN3 ?
How many moles is 114g NaN3? Calculate that.
then,you get 3/2 of those moles of N2.
how many liters is that (22.4 liters/mole)
so am i not using V=nRT/P
To solve this problem, you can follow these steps:
Step 1: Calculate the number of moles of NaN3.
Given that the molar mass of NaN3 is 65 grams/mol, divide the mass of NaN3 (114g) by its molar mass.
Number of moles of NaN3 = 114g / 65g/mol
Step 2: According to the balanced equation, 3 moles of N2 are produced for every 1 mole of NaN3.
Since the stoichiometric ratio is 3:1, multiply the number of moles of NaN3 by the stoichiometric ratio.
Number of moles of N2 = (114g / 65g/mol) * (3 mol N2 / 1 mol NaN3)
Step 3: Calculate the volume of N2 at STP.
At STP (Standard Temperature and Pressure), the volume of 1 mole of any gas is 22.4 liters.
So, multiply the number of moles of N2 by the molar volume at STP.
Volume of N2 = (114g / 65g/mol) * (3 mol N2 / 1 mol NaN3) * (22.4 L / 1 mol N2)
Step 4: Calculate the final volume of N2 in liters.
Plug in the calculated values into the equation:
Volume of N2 = (114g / 65g/mol) * (3 mol N2 / 1 mol NaN3) * (22.4 L / 1 mol N2)
Simplify the equation to get the final answer.
To find out how many liters of N2 gas are produced at STP (Standard Temperature and Pressure) when 114g of NaN3 decomposes, we can follow these steps:
Step 1: Determine the moles of NaN3. We will use the molar mass of NaN3 to convert grams to moles.
The molar mass of NaN3 is:
Na: 22.99 g/mol (sodium)
N: 14.01 g/mol (nitrogen)
3 × N: 3 × 14.01 g/mol = 42.03 g/mol
Total molar mass of NaN3: 22.99 g/mol + 42.03 g/mol = 65.02 g/mol
To calculate the moles of NaN3, divide the mass (114g) by the molar mass (65.02 g/mol) using the formula:
moles = mass / molar mass
moles = 114 g / 65.02 g/mol = 1.752 moles
Step 2: Apply the stoichiometry of the balanced equation to determine the moles of N2 gas produced.
From the balanced equation: 2 NaN3(s) ⟶ 2 Na(s) + 3 N2(g)
According to the stoichiometry, for every 2 moles of NaN3, 3 moles of N2 are produced. Therefore, we can set up a ratio to find the moles of N2:
(3 moles of N2 / 2 moles of NaN3) = (x moles of N2 / 1.752 moles of NaN3)
Simplifying the equation, we have:
x = (3/2) * 1.752 moles = 2.628 moles
Step 3: Convert the moles of N2 gas to liters at STP.
At STP, one mole of any ideal gas occupies 22.4 liters. Therefore, we can convert moles to liters using this conversion factor:
liters = moles * 22.4 L/mol
liters = 2.628 moles * 22.4 L/mol = 58.7832 L
Rounding off to an appropriate number of significant figures, we find that approximately 58.8 liters of N2 gas are produced at STP when 114g of NaN3 decomposes.