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1. I need to prepare a solution of 0.2 L 0.4 M then determine how many cm^3 of a solution of H2SO4 (sulfuric acid) 80.0% (density = 1.727 g/mL) should be diluted with H2O? Also also explain what's the pH of this solution if I combine 800 cm^3 of water and 6grams of sodium hydroxide?
When the reaction that occurs finally ceases, what will be the mass of unreacted copper in the bar? What will be the mass of silver metal that "plates out" of solution (that is, what mass of silver metal is produced by the reaction)
Three gases (8.00 g of methane, 18.0 g of ethane, and an unknown amount of propane were added to the same 10.0-L container. At 23.0 degrees C, the total pressure in the container is 4.50 atm. Calculate the partial pressure of each gas in the conta..
what is analytic
Calculate the amount of heat liberated (in kJ) from 405 g of mercury when it cools from 94.0°C to 14.0°C.
Using the van der Waals equation, calculate the pressure of 59.5 g of NH3 in a 5.20 L container at 47°C. The van der Waals constants for NH3 are: a = 4.17 L2xatm/mol2, b = 0.0371 L/mol.
How can I calculate the equilbrium constant and delta G and S given the enthalpy per mol of reaction and the final number of moles at equilbrium?
Using the van der Waals equation, calculate the pressure of 14.0 g of N2 in a 0.600 L container at 27.0 °C. The van der Waals constants
A 2.60 mole quantity of NOCl was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 22.0 percent of the NOCl had dissociated
The vapor pressure of pure ethyl bromide at this temperature is 400.0 torr. Assuming an ideal solution, what is the molecular mass of the compound?
The reaction: 2 HI → H2 + I2, is second order and the rate constant at 800 K is 9.70 × 10-2 M-1 s-1. How long will it take for 8.00 × 10-2 mol/L of HI to decrease to one-fourth of its initial concentration.
A cell composed of a platinum indicator electrode and a silver-silver chloride reference electrode in a solution containing both Fe2 and Fe3 has a cell voltage of 0.731 V.
Calculate the molar solubility of AgCl in a solution made by dissolving 10.0 g of CaCl2 in 1.00 L of solution.
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