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25.0 mL of ethanol initially at 7.0 degrees C is mixed with 35.0 mL of water initially at 25.3 degrees C in an insulated beaker. Assuming that no heat is lost, what is the final temperature of the
What product is formed when TWO equivalents of phenylmagnesium bromide (PhMgBr) are reacted with methyl salicylate (aka methyl-2-hydroxybenzoate)?
A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO. Determine the equilibrium pressure of each gas if Kp for the reaction at this temperature is 2.25.
You have 10 mL of calmagite (molecular weight 358.3g/mol). How much calmagite remains in an aqueous layer after a single 10 mL extraction of ethyl acetate (density 0.897 g/mL).
Calculate the concentrations of the H+ (or H3O+) ion in a 0.5 M HF solution
A piece of copper metal weighing 145 grams was heated to 100.0C and then dropped into 250. grams of water at 25.0 C. The copper metal cooled down, and the water became warmer until both were at a t
The temperature dependance of vapour pressure of solid sulfur dioxide is represented by log(p)= 10.5916- 1871.2(t) liquid sulfure dioxide log(p)= 8.3186 - 1425.7(T). Estimate the the temperature a
State three examples each of acids, bases, and salts commonly used in therapeutic processes. From the examples you state, select one acid, one base, and one salt and describe how and where they are
Nitrogen from gaseous phase is to be diffused in to pure iron at 7000 C. If surface concentration is maintained at 0.1% N, what will be the concentration 1 mm from the surface after 10 hours? The di
How are homogeneous mixtures in solution the same as homogeneous mixtures in suspension. How are homogeneous mixtures in solution the different from homogeneous mixtures in suspension.
What mass of sucrose (C12H22O11) should be combined with 494 g of water to make a solution with an osmotic pressure of 9.00 atm at 320 K?
The equivalent weight of a metal is double than that of oxygen. How many times is the weight of its oxide greater than the weight of metal ?
At a certain temperature the equilibrium constant for the reaction is 0.0255. What is the partial pressure of NO gas at equilibrium if the initial pressure of all the gases (both reactants and produ
At a given temperature, the equilibrium constant (Kp) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.172. If 0.224 atm N2O4 is sealed in a flask, what partial pressure of NO
Describe in details how we can determine the acid dissociation constant Ka for a week acid HA , include the description of the titration method and how determine the Ka from the reaction curve, then
If a solution of caffeine in chloroform (CHCl3) as a solvent has a concentration of 0.0870 m, calculate the following. (a) the percent caffeine by mass (b) the mole fraction of caffeine.
Demonstrate your systemic approach to find the pH of a solution where 1.0 x 10-8 mole of sodium acetate is dissolved in 1.0 L of water. (pKa of sodium acetate = 4.76)
At a constant volume and moles, the temperature of a sample of Neon (Ne) gas increased from 320*F to 370*C. what is the original pressure in atmosphere (atm) of the gas sample when the final pressur
How do you go about calculating the average deviation (step by step) using the following numbers:
A 1.26-g sample of an enzyme is used to make a 7.30-mL solution. What is the molar mass of the enzyme if the osmotic pressure of the solution at 298K is 0.138 ATM?
When you performed flame test on the chloride salts of several metallic element,you undoubtedly noticed that each element imparted a different color to the flame. these colors are characteristic fo
What are the molality of the solution and the molar mass of the solute? The freezing point of pure of benzene is 5.50°C and the Kf is 5.12.
A cell with .25 M internal concentration is placed into pure water. What is the pressure difference across the cell membrane?
Give two examples of elements or compounds that undergo sublimatiom. We studied the sublimation of elemental iodine under atmospheric pressure,iodine passes directly from the solid state to the vap
The reaction below was studied at a high temperature. At equilibrium, the partial pressures of the gases are as follows: PCl5 = 1.4 × 10-4 atm, PCl3 = 2.4 × 10-2 atm, Cl2 = 3.0 × 10-