(Solved): Experimental Data Mass of beaker + sodium carbonate (initial) Mass of empty beaker Mass of sodium c ...

Experimental Data Mass of beaker + sodium carbonate (initial) Mass of empty beaker Mass of sodium carbonate reactant Mass of beaker \( + \) sodium chloride (after heating) Co \( 6.699 \) Mass of sodium chloride product (experimental yield) \( 133.342 \) Data Analysis Use your data to experimental determine the mole-to-mole ratio between sodium carbonate and sodium chloride. Show your work for each step. B1. Convert the mass of sodium carbonate used to moles B2. Convert the mass of sodium chloride produced to moles Divide both of your results from the preceding two steps by the lower mole value to determine the simplest mole-to-mole ratio between sodium bicarbonate and sodium chloride. B3. Simplest mole ratio before rounding: moles \( \mathrm{Na}_{2} \mathrm{CO}_{3} \) : moles \( \mathrm{NaCl} \) B4. Simplest whole number mole ratio after rounding: 85. Using mass-to-mass stoichiometry, calculate the theoretical yield for reaction B. Use your initial mass of sodium bicarbonate reactant as a starting point, along with the relevant mole ratio from the balanced equation to perform this calculation. Show your calculations. B6. Calculate your percent yield of your sodium chloride product. Show your calculations. B7. List reasons why your observed percent yield may differ from your calculated theoretical yield of sodium chloride product.