The Martian atmosphere consists of approximately 96% carbon dioxide, and the mean molar mass is 43.34 g mol^-1 . The mean atmospheric pressure on the Martian surface is 6 hPa and the surface mean temperature is 210 K. What is the atmospheric pressure at 25 km from the ground (i.e. the top of Olympus Mons, a large volcano on Mars) in hPa? Use the gravity on Mars of 3.711 m s^-2 . Answer to two significant digits.

..........................................................................HCl – NaOH...........HNO3-NaOH

Initial Temperature from graph, oC...........................23.2......................24.1

Final Temperature from graph, oC............................36.75....................36.45

Temperature change, oC..........................................13.45....................12.35

Heat gained by solution, J.........................................13.6.....................12.4

Mass of solution, g....................................................104.4531.............94.5181

Specific Heat, J / g oC...............................................4.184...................4.184

...................................................................................NaCl...................NaNO3

Heat gained by the water solution in the surroundings..?.....................?

Heat capacity of calorimeter, J/oC...............................0.615 J/C..........0.615J/C

Heat gained by calorimeter, J.......................................?.......................?

Heat of neutralization, J...............................................?........................?

Moles of water formed in reaction................................?........................?

Molar enthalpy of neutralization...................................?........................?

Show a sample of each calculation performed. This calculation should include the math formula and the example with substituted values. All data should have proper significant figures and units. we placed 50 ml of 2.00M HCL into the inner cup. stired the solution untill the temperatew stabilized. placed 50 ml of 2.02 M NaOH into 100 m beake. pour the NaOH solution as completely as possible into the calorimeter with the first solution. we also did the same proces using 50 ml 2.00 M HNO3

You have .900 mol of H atoms in the ground state. How much energy is required to transition all of the atoms from the ground state to n=4

Calculate E

For the following reaction, 18.2 grams of iron are allowed to react with with 9.56 grams of oxygen gas.

I know this is multiple questions but it is in the same question on my HW and i'm so confused

What is the maximum amount of iron(II) oxide that can be formed? And What is the FORMULA for the limiting reagent? And What amount of the excess reagent remains after the reaction is complete?

1. The activation energy for the gas phase decomposition of dinitrogen pentoxide is 103 kJ.

N₂O_5--------- NO₂ + 1/2 O₂
The rate constant at 314 K is 2.76×10^-4 /s. The rate constant will be 1.49×10^-3 /s at -----------k

2. The activation energy for the gas phase decomposition of dinitrogen pentoxide is 103 kJ.

N₂O_5-----------2 NO₂ + 1/2 O₂
The rate constant at 305 K is 8.40×10^-5 /s. The rate constant will be ------- /s at 345 K.

What is a thermochemical equation? How is this different than a chemical equation? please appreciate typewriting when responding to this question  

How does these chemical equation balance, step by step? Why do they balance this way?

I already know how they balnace I just don't understand how they balance.

why does the O(2*) balance to 25? 2 C(8*)H(18*) + 25 0(2) yields 16 CO(2*) + 18 H(2*)O

These ones have me stumped as well

1 C(3)H(8) + 5 O(2) = 3 CO(2) + 4 H(2)O

Why does this equation balance this way?

1 Pb(OH)(2) + 2 HCl = 2 H(2)O + 1 PbCl(2)

Pb(OH)(2) + HCl + H(2)O + PbCl(2)

As I look at this equation, I am immediatly stumped because of the (OH). It kind of looks like it affects the whole equation, but I don't know why or know.

Please explain to me, in depth, why and how these equations balance this way

In a chemiluminescence lab do any factors completely stop light generation? If so, which ones?

How much copper, in weight percent, is in an alloy consisting of 94.1 at.% Ag and 5.9 at.% copper? The atomic weights for Ag and Cu are 107.87 g/mol and 63.55 g/mol, respectively.

Discuss the relationship between the production of nitrogen oxide species and the formation of ‘acid rain’ and the role played by carbon monoxide, methane, and the hydroxyl radical.

1.

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant.

2 HD(g) ↔ H2(g) + D2(g) Kc = 0.28
3 H2(g) + 3 D2(g) ↔ 6 HD(g) Kc = ?

2.

The reaction A(g)⇌2B(g) has an equilibrium constant of K = 0.070. What is the equilibrium constant for the reaction B(g)⇌12A(g)?

3.

Consider the reaction:
SO2Cl2(g)⇌SO2(g)+Cl2(g) Kp=2.91×10³ at 298 K
In a reaction at equilibrium, the partial pressure of SO2 is 158 torr and that of Cl2 is 307 torr .

Part A

What is the partial pressure of SO2Cl2 in this mixture?

PLEASE EXPLAIN HOW YOU GOT TO EACH ANSWER IN DETAIL. THANK YOU IN ADVANCE!

A 6.00  g sugar cube (sucrose: C12H22O11) is dissolved in a 350 mL teapot containing 80∘ C water (density of water at 80∘ C= 0.975 g/mL). What is the molality of the sugar solution?

Express the molality with the appropriate units.

Calcium chloride, CaCl2, is commonly used as an electrolyte in sports drinks and other beverages, including bottled water. A solution is made by adding 8.50  g of CaCl2 to 60.0 mL of water at 25∘C. The density of the solvent at that temperature is 0.997 g/mL. Calculate the mole percent of CaCl2 in the solution.

Express your answer as a percent to three significant figures.

Can someone please explain what a aug-cc-pVDZ basis set is in Physical chemistry using Gaussian?

A 2.687 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO3 and HCl aqueous solution. To this solution was added 1.900 grams of KI and 50.00 mL of a 0.00895 M KIO3 solution. The excess I3– was titrated with 50.00 mL of a 0.02000 M Na2S2O3 solution. What was the mass percent of arsenic trichloride in the original sample?