Final answer:
To find the mass of N2O5 resulting from the reaction, we can use the percent yield. The theoretical yield can be calculated using the stoichiometry of the balanced equation, and then multiplied by the percent yield to find the actual yield. In this case, the mass of N2O5 that will result from the reaction is 198.22 g.
Step-by-step explanation:
To find the mass of N2O5 resulting from the reaction, we need to use the percent yield. Percent yield is calculated by dividing the actual yield by the theoretical yield, and then multiplying by 100. In this case, the actual yield is unknown, but the percent yield is given as 61.1%. The theoretical yield can be calculated using the stoichiometry of the balanced equation. The balanced equation for the reaction is:
2 NO2 + N2O5 -> 4 NO2 + O2
From the balanced equation, we can see that 2 mol of NO2 react with 1 mol of N2O5. Therefore, for every 2 mol of NO2, we need 1/2 mol of N2O5. Since there are 6.0 mol of NO2, we need (1/2) * 6.0 = 3.0 mol of N2O5. To convert moles to mass, we use the molar mass of N2O5, which is 108.02 g/mol. Therefore, the mass of N2O5 that will result from the reaction is 3.0 mol * 108.02 g/mol = 324.06 g. However, this is the theoretical yield. To find the actual yield, we multiply the theoretical yield by the percent yield: 324.06 g * (61.1/100) = 198.22 g. Therefore, the mass of N2O5 that will result from the reaction is 198.22 g.