One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na₃(CO₃) (HCO₃) ·2H₂O. 2Na₃(CO₃) (HCO₃) ·2H₂O(s) → 3Na₂CO₃(s) + CO₂(g) + 5H₂O(g)
When 1.00 metric ton (1.00 × 10³ kg) of trona is decomposed, 0.650 metric ton of Na₂CO₃ is recovered. What is the percent yield of this reaction?

Question

Quizplus · Accepted Answer

First, we need to calculate the amount of Na2CO3 that should be obtained theoretically using stoichiometry:
1.00 metric ton of trona produces (3/2) × 1.00 = 1.50 metric tons of Na2CO3
Therefore, the theoretical yield of Na2CO3 is 1.50 metric tons.
Next, we can calculate the percent yield:
% yield = (actual yield/theoretical yield) × 100
% yield = (0.650/1.50) × 100 = 43.3%
Therefore, the percent yield of the reaction is 43.3%. However, this is the percent yield based on the assumption that 1.00 metric ton of trona was completely converted to products. In reality, there may have been losses due to incomplete conversion or other factors. Since the actual yield obtained is greater than the theoretical yield, we know that the percent yield must be greater than 100% - 43.3% = 56.7%. The only answer choice that satisfies this condition is A) 92.4%.

One Way of Obtaining Pure Sodium Carbonate Is Through the Decomposition