Consider the following data table, which is similar to the sort of data you will collect in this experiment. Complete the entries in the table. On graph paper from the end of this manual, construct a graph of the data, plotting the temperature change measured for each run versus the mumber of moles of substance A used for the run. Use your graph to determine the stoichiometric ratio in which substances A and B react. Explain your reasoning. 4. mL 1.0 MA mol of A mL 1.0 MB mol of B temperature change, °C 5.0 45.0 1.7 10.0 40.0 3.4 15.0 35.0 ·5.2 20.0 30.0 6.9 25.0 25.0 8.5 30.0 20.0 6.8 35.0 15.0 5.1 40.0 10.0 3.3 45.0 5.0 1.8

Consider the following data table, which is similar to the sort of data you will collect in this experiment. Complete the entries in the table. On graph paper from the end of this manual, construct a graph of the data, plotting the temperature change measured for each run versus the mumber of moles of substance A used for the run. Use your graph to determine the stoichiometric ratio in which substances A and B react. Explain your reasoning. 4. mL 1.0 MA mol of A mL 1.0 MB mol of B temperature change, °C 5.0 45.0 1.7 10.0 40.0 3.4 15.0 35.0 ·5.2 20.0 30.0 6.9 25.0 25.0 8.5 30.0 20.0 6.8 35.0 15.0 5.1 40.0 10.0 3.3 45.0 5.0 1.8

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...

See similar textbooks

Similar questions

Using the data provided: 2. Based on the temperature of the reaction, determine the partial pressure of the hydrogen gas collected. 3. Using the Ideal Gas Law, determine the experimental moles of hydrogen gas collected. 4. Calculate the % Yield of the reaction based on the actual yield (#3) and the theoretical yield (#1) calculations above.
blue. The reaction produces a reddish brown color copper metal and clear aluminum nitrate solution. Beaker Before Reaction Beaker After Reaction Blue colored solution Clear solution Silver piece of Al Small silver piece of Al Dark reddish brown solid According to the following data, what is the limiting reactant? Copper Nitrate solution, because the solution was blue at the end of the reaction showing some copper nitrate remained at the end of the reaction. Aluminum, because some Aluminum remained at the end of the reaction. Aluminum, because it was completely consumed in the reaction. Copper nitrate solution, because the solution was clear at the end showing it was completely consumed in the reaction.
Converting Concentrations to Different Units Introduction: Depending on how the concentration unit is defined, concentration can serve as a conversion between the amount of a solute and the amount of a solution or solvent. Concentrations can therefore be helpful in a number of stoichiometry issues. The original definition of the concentration unit is frequently preferred because it contains the conversion factor. Today, for chemists, it is suitable to make a solution in the lab using a specific concentration unit like molarity, and then convert the concentration to another unit. Today in the lab, I will prepare a sodium bicarbonate (baking soda) solution with a specific molarity. I will then translate the concentration into molality, mass percent, and mole fraction. Procedure The first step of this lab was to make sure I had everything I needed and that my surroundings were safe. I then looked at an empty beaker weighing paper and a balance. I first took a piece of weighing…
One important factor in any chemical synthesis is the actual quantity of desired product obtained compared to the theoretical amount predicted on the basis of the stoichiometry of the reaction. The ratio of the mass of product obtained to the theoretical quantity, expressed as a percentage, is referred to as the "percent yield" or more simply the "yield". For example: if we react HCl with excess NaOH one of the products will be NaCl. If we assume that all of the Cl in HCl ends up as NaCl we know that each mole of HCl consumed should produce a mole of NaCl product. Suppose that in a particular reaction 11.7 grams of HCl (36.5 g/mol) react with excess NaOH and 17.5 grams of NaCl (58.5 g/mol) are isolated from the reaction mixture by crystallization. What is the percent yield of NaCl in the experiement?
Hydrogen peroxide decomposes as shown below: 2 H2O2 → 2 H2O + O2 molar mass H2O2 = (34.0 g/mol) A sample of hydrogen peroxide solution was analyzed using the procedure from the “Enzymatic Decomposition and Analysis of Hydrogen Peroxide” experiment. A 5.89 g sample of the solution generated 0.0237 mol of oxygen gas. Calculate the grams of H2O2 in the solution.
When answering this problem, report the answer with the appropriate number of significant figures. When entering units, use proper abbreviated units with proper capitalization. A student followed the procedure in this experiment, using 48.92 mL of 1.00 molar HCl and 51.08 mL of 1.00 molar NaOH. Analysis of the collected data resulted in a heat transfer of 2808 J during reaction. Use this information to determine the heat of neutralization for this reaction in kJ/mol. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: ___________*10___ Units______
Mass of crucible and cover 12.73g 2. Mass of crucible, cover, and sample 24.11g 3. Mass of original sample 24.11- 12.73g= 11.97g 4. Mass of crucible, cover, and sample after 1st heating 20.01g 6. Mass of crucible, cover, and sample after 2nd heating (assume that this step was done) 19.98 g 7. Total mass lost by sample during heating what is the percentage of water in the sample? and what is the total mass lost by the sample?
The balanced equation for the decomposition of potassium chlorate is shown below. When carried out in lab, this reaction is found to produce 1.2 g of potassium chloride. For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this Information to make the requested calculation: 2 KCIO3(s) -> 2 KCI(s) + 3 02(g) 122.551 74.551 32 Determine the percent yield if the reaction consumes 0.50 kg of potassium chlorate:
She tells you that instead of titrating metal carbonates, it should be possible to react them with an excess of acid and collect the carbon dioxide gas that is generated by the reaction in a eudiometer. From the volume of carbon dioxide, you can calculate the moles of metal carbonate that reacted and use this information to determine the molar mass of the metal carbonate. She gives you a sample of another unknown metal carbonate to test this approach. You weigh out 0.1836 g of the unknown sample and react it with an excess of hydrochloric acid inside a eudiometer at 18.4 °C and 0.956 atm. Once the reaction is complete, you find that 17.20 mL of carbon dioxide gas were produced. a) How many moles of metal carbonate reacted? mol b) What is the molar mass of the metal carbonate? g/mol c) What is the chemical symbol of the metal cation?
11. How much iron, in kg, would need to be used in excess oxygen to produce 1,679 g of rust (iron(III) oxide)? use dimensional analysis to complete this question
Which of the following statements is true? (Several options can be specified.) a.The stoichiometric coefficient of a compound is the number in front of the compound in the reaction formula. The coefficient is negative for a reactant and positive for a product.b.Reaction heat is the heat development that occurs during a chemical reaction.c.When a gas is heated, the enthalpy content decreases.d.Entalpine changes during phase transformation (for example when iron melts or water evaporates).e.In an endothermic reaction, heat develops.
carbon 12.01 hydrogen 1.01 oxygen 16.00 A chemist will use a sample of 30 g of ethanol (CH3CH2OH) in an experiment. In one to two sentences, make and justify a claim about the number of moles of ethanol the chemist will use.