When 10.0 g of a mixture of Ca(ClO 3 ) 2 and Ca(ClO) 2 is heated to 700 °C in a 10.0-L vessel, both compounds decompose, forming O 2 (g) and CaCl 2 (s). The final pressure inside the vessel is 1.00 atm. (a) Write balanced equations for the decomposition reactions.

Hey everyone, we're told that gold medal and oxygen gas are produced when gold three oxide is decomposed at 160 to 290 degrees Celsius, they're requiring us to write the balanced chemical equation First. Let's get the formula for Gold three oxide. So we know that gold is A. U. And this has a plus three charge since we have that roman numeral three denoting that. And for oxide, we know that that's oxygen with a -2 charge since it's in our group six a. When we use our criss cross method, we end up with the formula of A. U. 203. So writing out our reaction, we have goal three oxide and we know that this is decomposed. So that means we produce gold medal plus oxygen gas. Now let's go ahead and balance this. Looking at our react inside, we have two of gold and three of oxygen. Looking at our product side, we have one of gold and two of oxygen balancing out our oxygen first. In our product side. If we add a coefficient of three prior to our oxygen gas we change our oxygen's into six. And so we can also change our react inside by adding a coefficient of two Prior to our goal three oxide. This changes our gold into four And our oxygen into six. Lastly we can balance out our gold in our product side by adding a four which will yield for gold. So this is going to be the balance equation for our reaction. I hope this made sense. And let us know if you have any questions.

Ch.10 - Gases: Their Properties & Behavior

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McMurry 8th Edition

Ch.10 - Gases: Their Properties & Behavior

Problem 141a

Chapter 10, Problem 141a

When 10.0 g of a mixture of Ca(ClO₃)₂ and Ca(ClO)₂ is heated to 700 °C in a 10.0-L vessel, both compounds decompose, forming O₂(g) and CaCl₂(s). The final pressure inside the vessel is 1.00 atm. (a) Write balanced equations for the decomposition reactions.

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Identify the chemical formulas for the compounds involved: Calcium chlorate is Ca(ClO_3)_2 and calcium hypochlorite is Ca(ClO)_2.

Write the balanced chemical equation for the decomposition of calcium chlorate: Ca(ClO_3)_2(s) \rightarrow CaCl_2(s) + 3O_2(g).

Write the balanced chemical equation for the decomposition of calcium hypochlorite: 2Ca(ClO)_2(s) \rightarrow 2CaCl_2(s) + O_2(g).

Note that both reactions produce calcium chloride (CaCl_2) as a solid and oxygen gas (O_2) as a product.

Ensure that the stoichiometry of each reaction is balanced, meaning the number of atoms of each element is the same on both sides of the equation.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Decomposition Reactions

Decomposition reactions occur when a single compound breaks down into two or more simpler products, often due to heat or other forms of energy. In this case, both calcium chlorate (Ca(ClO3)2) and calcium hypochlorite (Ca(ClO)2) decompose upon heating, releasing oxygen gas (O2) and forming calcium chloride (CaCl2). Understanding the specific products formed during decomposition is crucial for writing balanced chemical equations.

Balanced Chemical Equations

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation, adhering to the law of conservation of mass. Balancing equations involves adjusting coefficients to ensure that the number of atoms for each element is the same before and after the reaction. This is essential for accurately depicting the stoichiometry of the reaction and predicting the amounts of products formed.

Gas Laws and Pressure

Gas laws describe the behavior of gases in relation to pressure, volume, and temperature. In this scenario, the final pressure of 1.00 atm in a 10.0-L vessel indicates the amount of gas produced from the decomposition reactions. Understanding the ideal gas law (PV=nRT) helps in relating the pressure and volume of the gas to the number of moles produced, which is important for calculating the stoichiometry of the reactions.

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Open Question

Consider the combustion reaction of 0.148 g of a hydrocarbon with the formula CnH2n+2 in an excess of O2 within a 400.0-mL steel container. Before the reaction, the gaseous mixture had a temperature of 25.0 °C and a pressure of 2.000 atm. After complete combustion and heat loss, the products and excess O2 had a temperature of 125.0 °C and a pressure of 2.983 atm. (a) What is the formula and molar mass of the hydrocarbon? (b) What are the partial pressures in atmospheres of the reactants? (c) What are the partial pressures in atmospheres of the products and the excess O2?

Textbook Question

A mixture of CS21g2 and excess O21g2 is placed in a 10.0-L reaction vessel at 100.0 °C and a pressure of 3.00 atm. A spark causes the CS2 to ignite, burning it completely, according to the equation CS21g2 + 3 O21g2¡CO21g2 + 2 SO21g2 After reaction, the temperature returns to 100.0 °C, and the mixture of product gases (CO2, SO2, and unreacted O2) is found to have a pressure of 2.40 atm. What is the partial pressure of each gas in the product mixture?

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Textbook Question

When 10.0 g of a mixture of Ca1ClO322 and Ca1ClO22 is heated to 700 °C in a 10.0-L vessel, both compounds decompose, forming O21g2 and CaCl21s2. The final pressure inside the vessel is 1.00 atm. (b) What is the mass of each compound in the original mixture?

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Textbook Question

A 5.00-L vessel contains 25.0 g of PCl3 and 3.00 g of O2 at 15 °C. The vessel is heated to 200.0 °C, and the contents react to give POCl3. What is the final pressure in the vessel, assuming that the reaction goes to completion and that all reactants and products are in the gas phase?

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Textbook Question

A steel container with a volume of 500.0 mL is evacuated, and 25.0 g of CaCO₃ is added. The container and contents are then heated to 1500 K, causing the CaCO₃ to decompose completely, according to the equation CaCO₃(s) → CaO(s) + CO₂(g). (a) Using the ideal gas law and ignoring the volume of any solids remaining in the container, calculate the pressure inside the container at 1500 K.

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Textbook Question

A steel container with a volume of 500.0 mL is evacuated, and 25.0 g of CaCO₃ is added. The container and contents are then heated to 1500 K, causing the CaCO₃ to decompose completely, according to the equation CaCO₃(s) → CaO(s) + CO₂(g). (b) Now make a more accurate calculation of the pressure inside the container. Take into account the volume of solid CaO (density = 3.34 g/mL) in the container, and use the van der Waals equation to calculate the pressure. The van der Waals constants for CO₂(g) are a = 3.59 (L²-atm)/mol² and b = 0.0427 L/mol.

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When 10.0 g of a mixture of Ca(ClO3)2 and Ca(ClO)2 is heated to 700 °C in a 10.0-L vessel, both compounds decompose, forming O2(g) and CaCl2(s). The final pressure inside the vessel is 1.00 atm. (a) Write balanced equations for the decomposition reactions.

Verified video answer for a similar problem:

Key Concepts

Decomposition Reactions

Balanced Chemical Equations

Gas Laws and Pressure

When 10.0 g of a mixture of Ca(ClO₃)₂ and Ca(ClO)₂ is heated to 700 °C in a 10.0-L vessel, both compounds decompose, forming O₂(g) and CaCl₂(s). The final pressure inside the vessel is 1.00 atm. (a) Write balanced equations for the decomposition reactions.