What is the amount of oxygen needed to create output 20gm?
To determine the amount of oxygen needed to create an output of 20g, we need to know the stoichiometry of the reaction. The stoichiometry describes the balanced equation for the reaction, including the coefficients that indicate the number of molecules or moles of each reactant and product involved.
Since you didn't provide specific information about the reaction, it is difficult to give an exact answer. However, I can explain how you can calculate the amount of oxygen needed for a given reaction once you know the balanced equation.
1. Start by writing the balanced equation for the reaction. For example, let's say the reaction is the combustion of a hydrocarbon fuel: CxHy + O2 → CO2 + H2O.
2. Determine the molar ratio between the reactants and products. This is based on the coefficients in the balanced equation. In our example, the molar ratio between oxygen (O2) and carbon dioxide (CO2) is 1:1.
3. Convert the given amount of output (20g) to moles. To do this, divide the mass of the output by its molar mass. For example, if the output is CO2, the molar mass of CO2 is approximately 44g/mol. Hence, 20g CO2 would be 20g / 44g/mol = 0.45 mol CO2.
4. Use the molar ratio from step 2 to determine the amount of oxygen needed. In our example, if the molar ratio between O2 and CO2 is 1:1, then you would need 0.45 mol of O2 to produce 0.45 mol of CO2.
Remember, this is just a general explanation. The specific calculation will depend on the balanced equation of the reaction you are considering.