Use the Debye-Hückel equation to calculate the activity coefficient of each ion at the given ionic strength in an Ion Ion size (a, nm) aqueous solution at 25 °C. Pb2+ 0.450 Mg2+ Zn2+ 0.800 Cro- in a solution where u = 0.0317 M 0.600 Cro 0.400 3+ 0.900 PO 0.400 4+ 1.100 Ce+ 1.100 Ce+ in a solution where u = 0.0280 M

If an automobile travels 225 mi with a gas mileage of 20.5mi / gal,how many kilograms of CO{2} are produced? As- sume that the gasoline is composed of octane, C8H18(l) whose density is 0.69g / mL (b) Repeat the calculation for a truck that has a gas mileage of 5mi /gal

49.62 kcal into joules

CS2 6.61 Phosphoric acid, H,PO4, can be prepared by the reac- tion of phosphorus(V) oxide, P4O10, with water. P,O10(s) +H,O(1) → H,PO.(ag); AH = -96.2 kl What is AH for the reaction involving 1 mol of P4O10- %3D P,O 10(s) + 6H,O(I) 4H;PO,(aq)

1:39 1 Send a chat Enter your answer in the provided box. Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reaction CaF2 + H2SO4 → CASO4 + 2HF In one process, 5.75 kg of CaF, is treated with an excess of H,SO, and yields 2.45 kg of HF. Calculate the percent yield of HF. % yield

(2) 8. Write the balanced equation for the neutralization reaction between HI and Ba(OH)2 in aqueous solution. Include phases (physical states) in your equation. Use the arrow, not "=".

10) The number 0Aunpcired dectrans opected kr the Compler icn: ColoH)is: +

(3) A container holding NO2 and CO gas will lose NO2 gas via the reaction NO2 (g) + CO (g)  →  NO (g) + CO2 (g) A chemist measures the [NO2] over time and finds that plotting 1/[NO2 ]  versus time yields a straight line with a slope of 3.56×10-2 M-1·s-1.               If the container originally held 1.00 M NO2, what is the concentration of NO2 after 1.50 hour [NO2]1.5 hrs = ___________         How long will it take the [NO2] to drop to 20% of its initial concentration of 1.00 M?  T20% = __________

The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 71.0 mL of dioxygen gas are produced by this reaction, at a temperature of 50.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.

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