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When a 2.00-g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 1.717 kJ/K, the temperature decreases by 0.290 K. Calculate the molar heat of solution of KSCN.
Calorie contents of nuts, A cashew nut was burned and determined to have an energy value of 3.5Cal/g. The amount of nut burned was 0.9933g. How many of these nuts would a 67kg person have to eat to ob
What are the advantages of working with microscale equipment as opposed to larger equipment in a Williamson ether synthesis of phenacetin experiment.
This and the next question pertain to the following situation. A quantity of molecular hydrogen (H2) gas fills a one liter container at a temperature of 200 K and pressure of 1 atm.
A chemist has isolated a new natural product and determined its molecular formula to be C24H40O4. In hydrogenation experiments the chemist found that each mole of the natural product reacted with two
Calculate the quantity of heat released when 5.00 g of H2O2(l) decomposes at constant pressure.
Write a balanced chemical equation for the neutralization reaction upon which this titration is based, and indicate clearly which atom is being protonated.
Provide simple instructions for preparing 1.00 L of a solution having pH = 7.00 at 298 K. Your instructions should include the volumes of the solutions required.
Calculate the concentration of hydronium ions [H3O+] from the measured pH values. Express the answerin two significant figures. Please show how you got the answer.
What is the buffer capacity of the resulting solution? (The buffer capacity is the number of moles of NaOH that must be added to 1.0 L of solution to raise the pH by one unit.)
Draw a diagram of the electrochemical cell, labeling all electrodes and solutions. What is the pH in the Pt | H+ | H2 half-cell? What is the value of the equilibrium constant for the reaction occ
How many moles of carbon dioxide are contained in 7.75 grams of carbon dioxide.
The value of Delta g for the conversion of 3-phosphoglycerate to 2-phosphoglycerate (2PG) is +4.4 kj/mol. If the concentration of 3-phosphoglycerate at equilibrium is 2.55 mM, what is the concentrac
Question: Both HIO( Hypoiodous acid) and HIO3 (Iodic acid) are both weak acids. a. What is the oxidation state of the iodine atom in each acid?
The balanced equation for the combustion of ethanol is. How many grams of dioxygen are required to burn 5.9 g of C2H5OH?
Calculate ΔS (universe) for the decomposition of 1 mol of liquid water to form gaseous hydrogen and oxygen. Is this reaction spontaneous under these conditions at 25 °C?
When 5.00 g of fructose, C6H12O6, (FW 180.16 g/mol) is burned in a calorimeter whose heat capacity is 29.7 kJ/oK, the temperature increases by 2.635oK. Calculate the heat of combustion of fructose i
The temperature of moist air leaving the dehumidifier unit, in°C. The volumetric flow rate of air entering the air conditioner,in m3/min. The rate of water condensed, in kg/min.
Why does the introduction of a para nitro group have a much greater effect on the acidity constant of phenol than it does on benzoic acid? Justify your response by using appropriate resonance struct
Question: A sealed bottle of carbonated water (CO2 dissolved in water) has an initial pressure of 1.64 bar at 1 C. If the lid develops a small leak so that the system comes to equilibrium at PCO2 =
When 2.45g of an unknown weak acid (HA) with a molar mass of 85.0g/mol is dissolved in 250.0g of water, the freezing point of the resulting solution is -0.258 degrees C. Calculate Ka for the unknown
Why does the precipitate disappear when H2O is added? It is pushing the reaction to the left; why? It is not more reactant being added. It is changing Ksp but I thought only a change in temp would c
When 1.000g of tropinone is burned in a calorimeter with heat capacity of 25.950 kjC, the temperature increases from 25.262c to 25.993c. What is the change in enthalpy of tropinone?
What happened when CaCO3 was combined with hydrochloric acid? was a chemical reaction obvious here ? what about NaOH added to HCl? Was a reaction obvious in this case? Why indicators are important t
12.0 moles of gas are in a 3.00L tank at 22.7C. Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are a=2.300L^2*a