Given the two reactions

H2S⇌HS−+H+,   K1 = 9.24×10⁻⁸, and

HS−⇌S2−+H+,   K2 = 1.15×10⁻¹⁹,

what is the equilibrium constant Kfinal for the following reaction?

S2−+2H+⇌H2S

Part B

Given the two reactions

PbCl2⇌Pb2++2Cl−,   K3 = 1.74×10⁻¹⁰, and

AgCl⇌Ag++Cl−,   K4 = 1.26×10⁻⁴,

what is the equilibrium constant Kfinal for the following reaction?

PbCl2+2Ag+⇌2AgCl+Pb2+

What is the vapor pressure of a solution prepared by adding 50.0 g of NaCl to 250. g of pure water at 25 ^oC? (Water has a vapor pressure of 0.036atm at 25 ^oC)

Explain why either greatly decreasing or increasing the percentage of oxygen in the atmosphere is dangerous.

1)What are amino acids? Amino group, carboxyl end, what is the side chain of an amino acid?

2)What are essential and non-essential amino acid.

3)Which are the essential amino acids?

4)Classify the amino acids based on polarity of the R group:

1. The preparation of nanoparticle solutions adds a reducing reagent, sodium borohydride, to an oxidizing agent, hydrogen peroxide. Is it concievable that these two reagents would react with each other?

2. Why is it important to force the regression line in the Beer's Law plot of absorbance vs. concentration to go through the origin? Would adding the point (0,0) to your data set have the same effect? Why or why not?

I'm in intro chem so pleasee give in simple terms. Don't go too into depth

Methane gas (CH4) is burned in a combustor with a given percentage of excess air. The pressure and temperature of both the air and fuel are 101 kPa and 298 K respectively. Assume that the mole fractions are 79% nitrogen and 21 % oxygen for air (use M=28.97 kg/kmol and R=0.287 kJ/kg-K) and that water is a vapor in the exhaust. Given the values below, determine the following:

--Given Values--

m_fuel (kg) = 100

Excess Air = 25%

a) Determine the air fuel ratio (kmol_air/kmol_fuel) Answer=11.905 +/- 7.9E-02

b) Determine the amount (kmol) of fuel burned. Answer=6.2344 +/- 4.2E-02

c) Determine the amount (kmol) of air used. Answer=74.219 +/- 4.9E-01

d) Determine the amount (kmol) of CO2 produce Answer=6.2344 +/- 4.2E-02

e) Determine the amount (kmol) of H2O produced. Answer=12.4688 +/- 8.3E-02

f) Determine the amount (kmol) of N2 produced. Answer=58.6332 +/- 3.9E-01

g) Determine the amount (kmol) of O2 produced Answer=3.1172 +/- 2.1E-02

h) Determine the Enthalpy (kJ) of the reactants. Answer=-466646 +/- 3.1E+03

i) Determine the adiabatic flame temperature (K). Answer=2015.16 +/- 1.3E+01

j) Determine the Enthalpy (kJ) of CO2 in the products Answer=-1877561 +/- 1.3E+04

k) Determine the Enthalpy (kJ) of H2O in the products. Answer=-2099174 +/- 1.4E+04

l) Determine the Enthalpy (kJ) of N2 in the products. Answer=3323766 +/- 2.2E+04

m) Determine the Enthalpy (kJ) of O2 in the products. Answer=186323 +/- 1.2E+03

A 2.700×10−2 M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.3 mL . The density of water at 20.0∘C is 0.9982 g/mL.

Part A

Calculate the molality of the salt solution.

Express your answer to four significant figures and include the appropriate units.

Part B

Calculate the mole fraction of salt in this solution.

Gas experiement: Mg + HCl reaction

The volume of hydrgeon gas produced was not at standard temperautre and pressure. Convert the volume at the pressure and temperature of the experiement to a volume at standard temperature and pressure : STP (T=273.15 and P=1.00 atm).

Mg + 2HCl -> MgCl2 + H2

Mass of Mg: .012

Max pressure: 1.0946

Initial pressure: 1.0103

Pressure change: .0843

Temperature: 294.3

Used 5 ml of 1.0 M HCl in experiment

i mix 500ml of 0.250 M HCNO with 250ml of 0.333 M NaCNO. i then add 25ml of 1.00 M NaOH. A) how many moles of CNO- are in the beaker before the reaction takes place. B) what is the limiting reactant for the neutralization reaction

How does limestone react with SO2 to achieve removal of SO2 from exhaust gas stream?

BIOCHEMISTRY: Vmax and Km values

For the following problem

Sodium reacts with chlorine gas according to the reaction What volume of Cl2 gas, measured at 867 torr and 55.0 °C, is required to form 42.0 g NaCl (58.44 g/mol)

Give the maximum number of orbitals in an atom that can have these quantum numbers:

n = 3                                                   _______________

n = 3, l = 1                                           ______________

n=2, l=1, m_l= 0                                    _______________

n=0, l=0, m_l=0                                     _______________

Removing the electron from a Hydrogen atom corresponds to a raising the electron from n=1 to an orbit that has n=∞.

What is the energy needed to remove the electron from a hydrogen atom?

What is the energy in terms of kJ per mole?

What is the maximum number of orbitals that are specified by each set of quantum numbers

n=3, l=2, m_l = -2

n=1, l=0

n=5

n=2, l=2

n=5, l=3

n = 2

A piece of aluminum foil 1.00 cm square and 0.550 mm thick is dropped into bromine and reacts violently to form aluminum bromide solid. The density of aluminum is 2.699 g/cm³. A) Write a balanced equation for this reaction. B) If the reaction goes to completion, how many moles of aluminum reacted? C) How many grams of aluminum bromide formed, assuming the aluminum reacts completely?