calculate the total volume of gas at STP that is produced when 1gram of silver nitrate is heated in AgNO3=Ag+NO2+O2
Fist, balance the equation:
2AgNO3 → 2Ag + 2NO2 + O2
So, how many moles of AgNO3 in 1 gram?
You will get that many moles of NO2 and half that many of O2.
At STP, one mole occupies 22.4L
So now just crank it out.
Well, that's an explosive situation, isn't it? But fear not, my friend! Let the Clown Bot guide you through the hilariously scientific process!
To calculate the total volume of gas produced, we need to determine the number of moles of each gas. And to do that, we need to know the molar masses. Let's break it down:
The molar mass of AgNO3 (silver nitrate) is 169.87 g/mol.
The molar mass of Ag (silver) is 107.87 g/mol.
The molar mass of NO2 (nitrogen dioxide) is 46.01 g/mol.
The molar mass of O2 (oxygen) is 32.00 g/mol.
When 1 gram of AgNO3 is heated, it decomposes into Ag, NO2, and O2 in a 1:1:1 molar ratio. This means that for every one mole of AgNO3 decomposed, we get one mole of Ag, one mole of NO2, and one mole of O2.
Now, let the clownery begin!
Step 1: Convert the mass of AgNO3 to moles.
1 gram of AgNO3 / 169.87 g/mol = 0.00589 moles of AgNO3.
Step 2: Calculate the total moles of gas produced.
Since the molar ratio is 1:1:1, the moles of Ag, NO2, and O2 are all 0.00589 moles.
Step 3: Convert the moles of gas to volume at STP.
According to the ideal gas law, one mole of a gas occupies 22.4 liters at standard temperature and pressure (STP).
The total volume of gas produced = 0.00589 moles x 22.4 L/mole = 0.1318 liters (rounded to four decimal places).
So, when 1 gram of silver nitrate (AgNO3) is heated, it produces approximately 0.1318 liters of gas at STP. Remember to wear your clown nose for safety—a real gas explosion is no laughing matter!
To calculate the total volume of gas produced when 1 gram of silver nitrate (AgNO3) is heated, we first need to determine the balanced chemical equation for the reaction.
The decomposition of silver nitrate can be represented by the following equation:
2 AgNO3(s) → 2 Ag(s) + 2 NO2(g) + O2(g)
From the balanced equation, we can see that for every 2 moles of silver nitrate decomposed, 2 moles of nitrogen dioxide (NO2) gas and 1 mole of oxygen (O2) gas are produced.
Next, we need to convert the mass of silver nitrate to moles. The molar mass of silver nitrate (AgNO3) can be calculated as follows:
Molar mass of AgNO3 = Atomic mass of Ag + Atomic mass of N + (3 x Atomic mass of O)
= (107.87 g/mol) + (14.01 g/mol) + (3 x 16.00 g/mol)
= 169.87 g/mol
Using the molar mass, we can calculate the number of moles of silver nitrate:
Number of moles of AgNO3 = Mass of AgNO3 / Molar mass of AgNO3
= 1 g / 169.87 g/mol
≈ 0.00589 moles
Since the balanced equation shows that 2 moles of AgNO3 produce 2 moles of NO2 gas and 1 mole of O2 gas, we can determine the number of moles of gas produced.
Number of moles of NO2 gas = 2 x Number of moles of AgNO3
= 2 x 0.00589 moles
= 0.0118 moles
Number of moles of O2 gas = 1 x Number of moles of AgNO3
= 1 x 0.00589 moles
= 0.00589 moles
At Standard Temperature and Pressure (STP), 1 mole of any gas occupies 22.4 liters. Therefore, we can calculate the volumes of NO2 and O2 gas produced at STP.
Volume of NO2 gas at STP = Number of moles of NO2 gas x 22.4 liters/mol
= 0.0118 moles x 22.4 liters/mol
≈ 0.26432 liters (or 264.32 mL)
Volume of O2 gas at STP = Number of moles of O2 gas x 22.4 liters/mol
= 0.00589 moles x 22.4 liters/mol
≈ 0.131936 liters (or 131.94 mL)
Therefore, the total volume of gas produced at STP when 1 gram of silver nitrate is heated is approximately 0.26432 liters (or 264.32 mL) of nitrogen dioxide (NO2) gas and 0.131936 liters (or 131.94 mL) of oxygen (O2) gas.
To calculate the total volume of gas produced when 1 gram of silver nitrate (AgNO3) is heated, we need to use the balanced chemical equation for the decomposition of silver nitrate.
The balanced equation for the decomposition of silver nitrate is:
2AgNO3(s) → 2Ag(s) + 2NO2(g) + O2(g)
From the equation, we can see that for every 2 moles of AgNO3, we produce 2 moles of NO2 and 1 mole of O2.
Step 1: Calculate the number of moles of AgNO3
To determine the number of moles of AgNO3, we can use its molar mass. AgNO3 consists of one silver (Ag) atom, one nitrogen (N) atom, and three oxygen (O) atoms.
Ag: 1 x 107.87 g/mol = 107.87 g/mol
N: 1 x 14.01 g/mol = 14.01 g/mol
O: 3 x 16.00 g/mol = 48.00 g/mol
Total molar mass of AgNO3 = 107.87 + 14.01 + 48.00 = 169.88 g/mol
Number of moles of AgNO3 = Mass / Molar mass
Number of moles of AgNO3 = 1 g / 169.88 g/mol
Step 2: Calculate the number of moles of NO2 and O2 produced
From the balanced equation, we know that for every 2 moles of AgNO3, we obtain 2 moles of NO2 and 1 mole of O2.
Number of moles of NO2 = 2 x (Number of moles of AgNO3)
Number of moles of O2 = 1 x (Number of moles of AgNO3)
Step 3: Calculate the total volume of gas at STP
At Standard Temperature and Pressure (STP), one mole of any ideal gas occupies 22.4 liters.
Total volume of gas = (Number of moles of NO2 x 22.4 L/mol) + (Number of moles of O2 x 22.4 L/mol)
Now, substitute the calculated values of moles into the equation to find the total volume of gas produced at STP.