11:16 AM Sun Oct 22 Question 19 of 34 One of the commercial uses of sulfuric acid is the production of calcium sulfate and phosphoric acid. If 28.6 g of Ca3(PO4)2 reacts with 54.3 g of H₂SO4, what is the percent yield if 10.9 g of H3PO4 is formed via the UNBALANCED equation below? Ca3(PO4)2 (S) + H₂SO4 (aq) → H3PO4 (aq) + CaSO4 (aq) %
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![**Chemical Reaction and Percent Yield Calculation**
**Problem Statement:**
One of the commercial uses of sulfuric acid is the production of calcium sulfate and phosphoric acid.
If 28.6 g of \( \text{Ca}_3(\text{PO}_4)_2 \) reacts with 54.3 g of \( \text{H}_2\text{SO}_4 \), what is the percent yield if 10.9 g of \( \text{H}_3\text{PO}_4 \) is formed via the UNBALANCED equation below?
\[ \text{Ca}_3(\text{PO}_4)_2 (s) + \text{H}_2\text{SO}_4 (aq) \rightarrow \text{H}_3\text{PO}_4 (aq) + \text{CaSO}_4 (aq) \]
**Interface Explanation:**
Below the question, there is a keypad input area with numbers 0-9, a decimal point, a positive/negative toggle, a percent sign, and buttons for clearing input and a multiplication feature for powers of ten.
**Educational Context:**
This problem is designed to teach students how to calculate the percent yield of a chemical reaction using the provided chemical equation. The skill involves:
1. Balancing the given chemical equation.
2. Converting masses to moles using molar masses.
3. Determining the limiting reactant.
4. Calculating the theoretical yield.
5. Comparing the actual yield to the theoretical yield to find the percent yield.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F65936c84-20b2-4046-a438-4a3445f2d7a5%2F7bb8c7a4-9575-4a27-b18b-c0b864a28875%2F0cmlubam_processed.jpeg&w=3840&q=75)
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