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Calcium and Magnesium carbonates occur together in the mineral dolomite. Suppose you heat a sample of the mineral to obtain the oxides,CaO and MgO, and then treat the oxide sample with HCl. If 7.695g of the oxide sample requires 125 mL of 2,55 M HCl, CaO(s) + 2 HCl(aq)--->CaCl2(aq) + H2)(l) MgO(s) + 2HCl(aq)--->MgCl2(aq) + H2O(l) What is the weight percent of of each oxide (CaO and MgO) in the sample?
How much heat is evolved when 265 g of ammonia gas condenses to a liquid at its boiling point
For the compound MX, Ksp is 2.00 × 10-11. The anion X- forms the weak acid HX (Ka = 1.8 × 10-5). Calculate the solubility of MX in 10.00 M strong acid.
A container of gas at 760 mmHg and 20 degrees C is heated to 40 degrees C. What is the new pressure in mmHg?
The density at 20 degrees celsius of a 0.500 M solution of acetic acid in water in 1.0042 g/mL. what is the molality of the solution? the molar mass of acetic acide, CH3CO2H is 60.05 g
Calculate the molarity of a solution made by adding 44.4 mL of concentrated ammonia (28% by mass, density 0.880 g/mL) to some water to some water in a volumetric flask
When pure carbon burns in air, 10.0 kg of carbon react with the oxygen in the air to form 36.7 kg of carbon dioxide. Calculate the percentage of oxygen contained in carbon dioxide.
The compound is involved in the citric acid cycle for energy production within the cell. However, the compound is unstable and slowly decomposes spontaneously. Draw the decomposition products.
How much thermal energy transfer is required to vaporize 1.0 metric tone of ammonia?(1 metric ton = 10^3Kg). The delta H vaporization for ammonia is 25.1KJ/mol.
Suppose that for the precipitation of the stock solution of borzac, the solid borax reagent is contaminated with a water-souble substance that does not eact with HCl.
a line in the Balmer series of hydrogen has a wavelength of 434 nm from what state did the electron originate
A 370. mL air sample collected at 35°C has a pressure of 550. torr. What pressure will the air exert if it is allowed to expand to 425 mL at 49°C.
2 FeS + 3 N2 → 2 FeN + 2 SN2 This reaction has a 65.0% yield. How much N2 is consumed if 13.6 g of FeN are produced?
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