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?

검증된 단계별 안내

Step 1: Write the balanced chemical equations for the decomposition of each compound. For calcium chlorate (Ca(ClO3)2), the decomposition reaction is: Ca(ClO3)2(s) → CaCl2(s) + 3O2(g). For calcium chlorite (Ca(ClO2)2), the decomposition reaction is: Ca(ClO2)2(s) → CaCl2(s) + 2O2(g).

Step 2: Use the ideal gas law to determine the total moles of O2 produced. The ideal gas law is PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in Kelvin.

Step 3: Let x be the moles of Ca(ClO3)2 and y be the moles of Ca(ClO2)2. From the stoichiometry of the reactions, the total moles of O2 produced can be expressed as 3x + 2y. Set up the equation 3x + 2y = total moles of O2 from Step 2.

Step 4: Convert the masses of Ca(ClO3)2 and Ca(ClO2)2 to moles using their molar masses. Set up the equation x * molar mass of Ca(ClO3)2 + y * molar mass of Ca(ClO2)2 = 10.0 g (total mass of the mixture).

Step 5: Solve the system of equations from Step 3 and Step 4 to find the values of x and y. Convert these moles back to grams to find the mass of each compound in the original mixture.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

19m

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this question, stoichiometry will help relate the masses of the original compounds to the moles of products formed during decomposition.

Gas Laws

Gas laws describe the behavior of gases in relation to pressure, volume, and temperature. The ideal gas law (PV=nRT) is particularly relevant here, as it allows us to relate the pressure of the gas produced to the number of moles and the volume of the container. Understanding these relationships is crucial for determining how the decomposition of the compounds affects the final pressure in the vessel.

Decomposition Reactions

Decomposition reactions involve a single compound breaking down into two or more simpler products, often requiring heat. In this scenario, both calcium hypochlorite (Ca(ClO)2) and calcium chloride (CaCl2) decompose upon heating, producing oxygen gas and solid calcium chloride. Recognizing the products of these reactions is essential for calculating the mass of each compound in the original mixture.