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What is the equivalent mass of metal that is dissolved in sulfuric acid during hydrogen release if 2.27 g metal reacts with 30 ml 33 w/w% H2SO4 (density 1.25 g/cm^3, molar mass is 98 g/mole)?
If 45 mL of H2 (g) are collected over water at 27°C and 751 mmHg external pressure. How many grams of Al were reacted.
Compare the release of S02 in the scrubbed flue gas (determined in Problem 14.6) with the EP A limit of no more than 520 nanograms S02 per joule of heat input to the boiler.
On average, cow milk is 4.7%(w/w) lactose. The molecular weight of this disaccharide is 342.3g C12H22011. Assuming milk has the density of water.
What is the free Zn2+ concentration if 0.020 M Zn2+ solution is mixed with an equal volume of 2.0 M NH3? Kf for [Zn(NH3)4]2+ is 4.1 × 10^8
A student found that her mixture was 15% NH4Cl, 20% NACL, and 75% SiO2. Assuming her calculations are correct, what did she most likely do incorrectly in her experiment?
How many liters of gas could be generated at STP from the reaction of dilute with 15.55 of an ore that is 29.7 iron(II) sulfide by mass?
You dissolve 650.0 g of sugar (C12H22O11) in 726 mL of water. The density of wat is 1.00 g/mL.
When a 2.3L sample of hydrogen gas at 25oC is heated to 120oC at constant pressure, what is the new volume of the gas?
You are given the chemical reaction (unbalanced equation): AsF3 + C2Cl6 AsCl3 + C2Cl2F4, if 1.3618 mol of AsF3 are allowed to react with 1.000 mol of C2Cl6, what would be the theoretical yield of C2Cl2F4, in grams?
Enter the molecular, ionic and net ionic equation for the following reactioins. I am having trouble figuring out when to make the water molecule and when not to.
In an oxidation-reduction reaction, it required 25.6 ml of a 0.65 M potassium permanganate solution to reach the equivalence point with 15.0 mL of an iron(II) sulfate solution.
If the water in your house has 1000.0 mg/L of calcium carbonate dissolved in it, How many grams of sodium oxalate could you mix with 100.0 mL of that water before a precipitate would form.
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