4. Determine the final temperature of the solution formed when 0.31 g sodium oxide is added to100 ml water in a calorimeter. Assume that the volume of the resulting solution is 100 ml. Thetemperature before reaction is 19°C. The heat capacity of the calorimeter is 20J/°C. Supposethat the specific heat and density of the solution are the same as those of water.Write down all the reaction equations needed to solve this exercise.

To solve this problem, you need to consider the heat exchange between the sodium oxide (Na₂O) and…

Answered: 4. Determine the final temperature of…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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When calculating enthalpy of reaction values, we use the "products minus reactants" mathematical model. Which explanation of this model is most correct? A) The products are coming into existence, thus we use their enthalpy of formation. The reactants are ceasing to exist, thus we use the opposite of their enthalpy of formation. B) "Products minus reactants" is an equation, not a model, and thus tells us nothing about the reaction. C) We model the chemical reaction as taking reactants and turning them into products. The exact steps don't matter as long as it comes to the product eventually. That is why we use "products minus reactants." D) We model the reaction as taking reactant molecules and dispersing them in to pieces (the opposite of the formation reaction of the reactants) and taking those pieces and condensing them down into products (the same as the formation reaction for those products.) Thus we take the negative of the enthalpy of formation for the reactants and…
A 5.90-g chunk of potassium is dropped into 1.00 kg water at 24.7°C. What is the final temperature of the water after the preceding reaction occurs? Assume that all the heat is used to raise the temperature of the water.
A decomposition of hydrogen peroxide into water and oxygen gas is an exothermic reaction. If the temperature is initially 28˚ C, what would you expect to see happen to the final temperature? Explain what is happening in terms of energy of the system and the surroundings. endothermic or exothermic?
Is oxygen a reactant or product in a combustion reaction? Are combustion reactions exothermic or endothermic?
A certain chemical reaction releases 33.8/kJg of heat for each gram of reactant consumed. How can you calculate what mass of reactant will produce 810.J of heat? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols.
Differentiate the enthalpy of a solution with the enthalpy of combustion or a reaction. Also, give the importance of the enthalpy of a solution and why it must be measured.
4. The specific heat of water is quite high at 4.184 J/gC. Explain how life on this planet would be different if the specific heat of water were that of lead at 0.128 J/gC.
4. A 505 gram piece of copper tubing is heated to 99.0 °C and placed in an insulated vessel containing 59.8 grams of water at 24.8 °C. Assume that the water and the vessel are at the same temperature and that all of the heat released from the copper is absorbed by the water and the vessel. If the vessel has a heat capacity of 10.0 J/K, what is the final temperature of the system when it reaches physical equilibrium?
A 8.27 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. If -3.19 x 103 J of heat was lost during the dissolution reaction of 0.0708 moles of the unknown salt, what is the enthalpy change (in kJ/mol of salt) for the dissolution reaction?
A 45.90 g sample of pure copper is heated in a test tube to 99.40°C. The copper sample is then transferred to a calorimeter containing 61.04 g of deionized water. The water temperature in the calorimeter rises from 24.51°C to 29.10°C. The specific heat capacity of copper metal and water are J and 4.184 J respectively. g• °C 0.387 g• °C Assuming that heat was transferred from the copper to the water and the calorimeter, determine th heat capacity of the calorimeter. Heat capacity of calorimeter =
In an endothermic reaction the enthalpy of the reactants is greater than the enthalpy of the products. In an endothermic reaction, the energy required to break existing bonds is more than the energy released when new bonds form. In an exothermic reaction the energy required to break existing bonds is less than energy released when new bonds form. In an exothermic reaction the potential energy of the reactants is higher than the potential energy of the products and the energy term would be written on the product side of the equation.
Calculate the change in energy for the following processes and identify if the process is endothermic or exothermic. 1. How much heat is released by a system when 45 J of work is done on it to decrease its energy to 23 J? 2. What is the work done by a system when it absorbs 47 J of heat and gain 12 J of energy? 3. A gas absorbs 51 J of heat as it does 96 J of work. with explanation and solution please.

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