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1. What is the empirical formula of a compound composed of 3.25% hydrogen (H), 19.36% carbon (C), and 77.39% oxygen (O) by mass? 2. A compound with the empirical formula CH2 has a molar mass of 84 g/mol. What is the molecular formula for this compound? 3. A 15.85 g sample of Mo2O3(s) is converted completely to another molybdenum oxide by adding oxygen. The new oxide has a mass of 16.91 g. Add subscripts below to correctly identify the empirical formula of the new oxide. 4. A 7.99 g sample of a compound contains 2.55 g potassium (K), 2.31 g chlorine (Cl), and oxygen (O). Calculate the empirical formula. 5. A compound is 54.53% C, 9.15% H, and 36.32% O by mass. What is its empirical formula? 6. The molecular mass of the compound is 132 amu. What is the molecular formula? 7. How many grams of a 14.0% sugar solution contain 38.5 g of sugar? 8. You need to dissolve CaCl2 in water to make a mixture that is 33.0% calcium chloride by mass. If the total mass of the mixture is 741.4 g, what masses of CaCl2 and water should be used? ( Mass of CaCl2) ( Mass of H20) 9. A solution contains 4.40 g of solute in 11.6 g of solvent. What is the mass percent of the solute in the solution? 10. A 4.68 g sample of a laboratory solution contains 1.32 g of acid. What is the concentration of the solution as a mass percentage? 11. How many moles of NaOH are present in 19.0 mL of 0.280 M NaOH? 12. Calculate the number of moles of solute in 93.83 mL of 0.1595 M K2Cr2O7(aq). 13. The mass percentage of hydrochloric acid within a solution is 40.00%. Given that the density of this solution is 1.200 g/mL, find the molarity of the solution. 14. How many grams of solute are present in 835 mL of 0.710 M KBr? 15. calculate the molarity a) 21.7 g of NaCl in 799 mL of solution. = in (M) b) 0.500 mol of NaOH in 1.40 L of solution.= in (M) 16. Calculate the molarity a) 0.250 mol of Na2S in 1.80 L of solution. b) 34.7 g of MgS in 911 mL of solution. 17.How many milliliters of 12.0 M HCl(aq) are needed to prepare 915.0 mL of 1.00 M HCl(aq)? 18. What is the concentration of a solution made by diluting 35 mL of 6.0 M HCl to a final volume of 750 mL?
find out the molecular formula and empirical of this compound and determined to contain 4.36 grams of phosphorus and 5.64 grams of oxygen
Which of the following compounds is expected to have the highest boiling point? octane, 2,3-dimethylhexane, 2,2,3,3-tetramethylbutane
The atmospheric sulfur dioxide concentration over a certain region is 0.12 ppm by volume. Calculate the PH of the rainwater due to this pollutant. Assume the dissolution of SO2 does not affect its pressure.
Suppose in universe Xacto matter is composed of protons, neutrons, and special matter X. For elements in a, design and draw a new periodic table that makes sense for this parallel universe.
determine the actual yield If the percent yield of the reaction in B was 91% describes the oxidation of ethanol (C 2 H 5 OH) to acetic acid (CH 3 COOH) by potassium permanganate (KMn04
A 1-ft-diameter cylinder is closed on one end and fitted with a moveable piston on the other. With 1 atm applied pressure, the piston is located 20 ft from the closed end
Suppose that you wished to prepare copper(II) carbonate by a precipitation reaction involving Cu2+ and CO32-. Select all of the pairs of reactants that could be used as solutes
at 90C the foll equilibrium is established, H2(g) + S(s)=H2S(g) K=6.8*10-2 If 0.2 mol of hydrogen and 1 mol of sulphur are heated to 90C in a 1L vessel.
A mixture of CO2 and N2 gases has an experiment density of 21922 mol/m3 at T=225K and Pressure= 68.759 MPa and Z=1.67661. What is density of this mixture of gases in mol/m3 by Peng-Robinson equation of state? (Mole fraction of Co2= 10.56%)
Calculate the concentrations of all species at equilibrium for the following case.
What is the concentration of the vitamin C standard solution? Using a balance, 125mg of Vitamin C was weighed out and was added to a 100-mL beaker and dissolved in 50mL of DI water.
Calculate the molar solubility of AgBr in a 1.00 M aqueous solution of ammonia. Then calculate the solubility of AgBr in pure water, and compare the two solubilities. (Ksp for silver bromide is 7.7x10 -13 and Kf for Ag(NH3)2+ is 1.6x10^7)
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