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Consider the following hypothetical reaction: X(g) -----> Y(g) A 200.0-mL flask is filled with 0.120 moles of X. The disappearance of X is monitored at timed intervals. Assume that temperature and volume are kept constant. The data obtained are shown in the table below. Time (min) 0 20 40 60 80 moles of X 0.120 0.103 0.085 0.071 0.066 (b) Calculate the average disappearance of X in M/s in the first two 20-minute intervals. (c) What is the average rate of appearance of Y between the 20- and 60-minute intervals?
how many grams of sugar are in 15.0% concentrated solution with a total mass 125 g?
Green light of a wavelength 516 nm is absorbed by an atomic gas. What is the energy difference between the two quantum states involved in the transition.
Cadmium ion in solution is analyzed by precipitation as the sulfide, a yellow compound used as a pigment in everything from artists' oil paints to glass and rubber. Calculate the molar solubility of cadmium sulfide at 25?C ?
if the height of the mercury column in a leveling bulb is 30 mm greater than that in the gas buret and atmospheric pressure is 670 mm, what is the pressure on the gas trapped in the buret.
A 29.20 g piece of iron and a 25.30 g piece of gold at 100.0 degree C were dropped into 980.0 mL of water at 15.65 degree C. The molar heat capcities of iron and gold are 25.19 J/(mol degree C) and 25.41 J/(mol degree C), respectively.
A rigid tank contains 1.50 moles of an ideal gas. Determine the number of moles of gas that nust be withdrawn from the tank to lower the pressure of gas from 25atm to 35 atm.
How to Name and Define Acids, How can you know that HNO3 is nitric acid and HNO2 is nitrous acid? How do you know the difference in endings?
A soft drink contains 35 mg. of sodium in 315g. of H2O. What is the concentration of sodium in the soft drink in mass percent?
Calculate the mass in grams of carbon dioxide that will be produced when 25.0 g of ethanol is burned.
Write the corresponding ionic and net ionic equations after Balancing these given equations
Calculate the empirical formula for a chemical compound which gives the following analysis: 12.6 percent lithium, 29.2 percent sulfur, and 58.2 percent oxygen.
Consider the following electrochemical cell at 298 K. One compartment contains a 1.00-M solution of silver nitrate. The other compartment contains a saturated solution of silver iodide
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