What volume of oxygen gas is produced when 17.5 grams of KBrO3 decomposes?

and the equation is KBrO3==>KBr+30

HELP ME PLZ

Where did you get that reaction equation? Atomic O is not stable product

The reaction is actually
2 KBrO3 -> 2 KBr + 3 O2

Calculate the number of KBrO3 moles you start with, using the molar mass; then take 3/2 that number as the number of moles of O2 that form. Call it n.

The use V = n R T/P for the volume V

You need to specify the absolute temperature T and pressure P. At 0 C and 1 atm, each mole occupies 22.4 liters.

I'll be glad to critique your work.

To determine the volume of oxygen gas produced when 17.5 grams of KBrO3 decomposes, we need to use the given equation and the concept of stoichiometry.

Step 1: Find the molar mass of KBrO3.
The molar mass of KBrO3 can be calculated by adding up the atomic masses of each element in the compound.
K (potassium) = 39.10 g/mol
Br (bromine) = 79.90 g/mol
O (oxygen) = 16.00 g/mol (two atoms of oxygen in KBrO3)
Total molar mass of KBrO3 = (39.10 g/mol) + (79.90 g/mol) + (16.00 g/mol x 3) = 167.10 g/mol

Step 2: Use the molar mass of KBrO3 to convert grams to moles.
Moles = Mass / Molar mass
Moles of KBrO3 = 17.5 g / 167.10 g/mol ≈ 0.105 mol

Step 3: Determine the stoichiometric ratio between KBrO3 and O2 using the given equation.
From the balanced equation: 2 moles of KBrO3 decompose to produce 3 moles of O2.
So, the ratio is 2:3.

Step 4: Calculate the moles of oxygen gas produced.
Moles of O2 = (Moles of KBrO3) x (3 moles of O2/2 moles of KBrO3)
Moles of O2 = 0.105 mol x (3/2) = 0.1575 mol

Step 5: Convert the moles of oxygen gas to volume using the ideal gas law.
The ideal gas law states PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Since we do not have the values for pressure, temperature, or volume, we cannot directly calculate the volume.

You will also need to know the temperature and pressure conditions to calculate the volume of oxygen gas accurately. Make sure you have these values before proceeding.

Please note that the volume of a gas also depends on pressure and temperature.