A swimming pool in the neighborhood of a smelter receives atmospheric SO2 deposition. The average concentration over the pool is 300 micrograms SO2/m3. If SO2 deposition velocity is 1.2 cm/sec and all SO2 deposited on the pool is transformed to H2SO4,how much NaOH must be added to the pool (moles per square meter of surface area) weekly to neutralize the H2SO4 and prevent the pool from becoming acidified?

Write the balanced neutralization reaction between H2SO4 and KOH in aqueous solution. Phases are optional.

0.450 L of 0.490 M H2SO4 is mixed with 0.400 L of 0.210 M KOH. What concentration of sulfuric acid remains after neutralization?

How do you write molecular formulas for compounds? How do you identify if they are ionic or covalent? Please use the following as examples: Copper (I) sulfide / Sulfer tetrafluoride

Hydrobromic acid dissolves solid iron according to the following reaction:
Fe(s)+2HBr(aq)?FeBr2(aq)+H2(g)

What mass of HBr (in g) would you need to dissolve a 3.0?g pure iron bar on a padlock? Express your answer using two significant figures. m=______________g

What mass of H2 would be produced by the complete reaction of the iron bar?

Express your answer using two significant figures. m=_____________________g

A beaker containing 50.0 mL of 0.300 M Ca2+ at pH 9 is titrated with 0.150 M EDTA. The pCa2+ at the equivalence point is

(a) Select all of the correct statements about reaction rates from the choices below.

The lower the rate of a reaction the longer it takes to reach completion.


A balanced chemical reaction is necessary to relate the rate of reaction to the concentration of a reactant.


The rate of a fast step has more effect on the overall reaction rate than the rate of a slow step.


Solid catalysts increase reaction rates as their surface areas increase.


Slow reactions can be speeded up by raising the temperature.


Reactions involving very unstable combinations of chemicals have small rate constants.


Reaction rates always increase as masses of solid reactants increase.

2.90 moles of an ideal gas with Cv,m = 3R/2 undergoes the transformations described in the following list from an initial state described by T=310. K and P = 1.00 bar.

Part 1) The gas is heated to 725K at a constant external pressure of 1.00 bar. calculate q, w, delta U, delta H and delta S for this process.

Part 2) The gas is heated to 725 K at a constant volume corresponding to the initial volume. calculate q, w, delta U, delta H, delta S for this process

Part 3) the gas undergoes a reversible isothermal expansion at 310.K until the pressure is one third of its initial value. calculate q, w, delta U, delta H, delta S for this process

Balance the following reactions in acidic conditions. show all steps.

A). Mno4^-1 + C2O4^-2 --------- MnO2 + CO2

B). Br2 --------- Br^-1 + BrO^-1

C). Cu + NO3^-1 ---------- Cu^+2 + NO

D). MnO4^-1 + S^-2 --------- MnO2 + S

A mixture of 1.71 moles of B and 1.23 moles of C is placed in a 1.00 liter container at a given temperature and allowed to reach equilibrium according to the following equation. Calculate [A] present at equilibrium. Calculate [A] with 3 significant figures, exponential notation, and no units.

2A <----> B + C     K_c= 3

What is the vapor pressure of a solution made by adding 25.0 g of glucose, C6H12O6 (molar mass = 180. g/mol) to 145 g of water and heating the solution to 60 °C? The vapor pressure of pure water at 60 °C is 149 torr. The vapor pressure of pure glucose at 60 °C is negligible.

(a) 2.53 torr

(b) 127 torr

(c) 143 torr

(d) 146 torr

Consider the titration of a 21.0 −mL sample of 0.110 M HC2H3O2 with 0.125 M NaOH. Determine the pH after adding 6.00 mL of base beyond the equivalence point.

Calculate the equilibrium concentrations of N2O4 and NO2 at 25 degrees celcius in a vessel that contains an initial N2O4 concentration of 0.0500M. The equilibrium constant Kc for the reaction N2O4 (g) (equilibrium arrows here) 2NO2(g) is 4.64 x 10-3 at 25 degrees Celcius.

4.60 mol of solid A was placed in a sealed 1.00-L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.20 M, where it remained constant.

A (s) <---> B (g) + C (g)

Then, the container volume was doubled and equilibrium was re-established. How many moles of A remain?

Please break down the steps so I can see how to solve. Thank you!

Urea (CH4N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NH3) with carbon dioxide as follows:

2NH3(aq)+CO2(aq)→CH4N2O(aq)+H2O(l)

In an industrial synthesis of urea, a chemist combines 129.2 kg of ammonia with 211.4 kg of carbon dioxide and obtains 180.1 kg of urea.

1).Determine the theoretical yield of urea

2).Determine the percent yield for the reaction.

Write the net ionic equations that occur in the following cells:

1. Pb/Pb²⁺ // Ag⁺/Ag

2. Zn/Zn²⁺ // Pb²⁺/Pb

3. Al/Al³⁺ // Cd²⁺/Cd