Suppose 8.00 g of calcium chloride are mixed with 6.00 g potassium hydroxide. What is in the container after the reaction?

The answer is below but please explain how to solve this problem.

Answer: no potassium hydroxide left; 2.86 g calcium chloride left; 3.96 g calcium hydroxide and 7.98 g potassium chloride

For Gorilla glass, Xensation, Sapphire glass, and Dragontrail glass, how they are made and processed, their hardness, strength, and cost. In metric please.

Mass of metal slug (measure once and use for both runs) 49.614 g 54.687 g Mass of water in calorimeter cup 80.113 g 80.087 g Initial temperature of water in the calorimeter 22.0 ºC 22.0ºC Initial temperature of the metal (assume 100.0 ºC) ____________ºC _____________ºC Equilibrium temperature of the metal + water 26.8 ºC 26.6ºC in the calorimeter ΔTwater ____________ºC ____________ºC ΔTmetal ____________ºC _____________ºC qwater * (S.H.C.water = 4.184 J/ g °C ) ____________J _____________J qmetal ** ____________J _____________J Calculated specific heat capacity of the metal ____________ J /g°C ____________ J /g°C B. Enthalpy of Reaction (Dissolution) CaCl2 NH4NO3 Mass of water in calorimeter cup 100.00 g 100.00g Mass of solid compound used 10.026 g 10.041g Mass of solution formed ____________g _____________g Initial temperature of water 22.0ºC 22.0ºC Max (if it rises) or min (if it falls) temperature of solution 38.2ºC 15.1ºC ΔTsoln (use initial temp. of water for initial temp. of soln.) ____________ºC _____________ºC qsoln (assume S.H.Cof soln. = S.H.C. of water) ____________J _____________J qreaction (amount of heat absorbed by the reaction)* ____________J _____________J “Heat of solution” ** ____________J/g _____________J/g ΔrH *** ____________kJ/mol_____________kJ/mol Is the dissolution reaction exothermic or endothermic? ____________ _____________ Enthalpy of Reaction (Neutralization) Initial temperature of HCl solution 22.0ºC Initial temperature of NaOH solution 23.2ºC Final temperature of neutralized mixture 29.4ºC ΔT (for the initial temperature, average the initial temperatures of the HCl and NaOH) ____________ºC qsoln (assume all the heat is absorbed by 104 g soln.) ____________J qrxn for the neutralization reaction ____________J Number of moles of H2O formed by the reaction ____________mol ΔHr (in kJ per mole of H2O formed by the reaction) ____________kJ/mol Is the neutralization reaction exothermic or endothermic? _____________

1) How many photons are emitted during a transition from a higher level orbit to a lower level orbit? a)1 b)2 c)3 d)4

2) True/False? An electron can transition from any allowed orbit to any other allowed orbit.

3) What is the wavelength of light emitted when an electron drops from the 3 to the 2 shell in a hydrogen atom?

1) Complete and balance the following half-reaction: H2SO3(aq)?SO2?4(aq) (acidic solution)

2)Complete and balance the following half-reaction:

NO?3(aq)?NO(g)(acidic solution)

3)Complete and balance the following half-reaction:

O2(g)?H2O(l)(acidic solution)

4)Complete and balance the following half-reaction:

O2(g)?H2O(l) (basic solution)

5)Complete and balance the following half-reaction: Mn2+(aq)?MnO2(s) (basic solution)

6)Complete and balance the following half-reaction: Cr(OH)3(s)?CrO2?4(aq) (basic solution)

When the following equation is balanced with the smallest integral coefficients, the coefficient of the HCl(g) is ______.
H₂O(l) + SO₂Cl₂(l) → HCl(g) + SO₃(g)

Given the reaction: 2 Al (s) + 6 HNO₃ (aq) ® 2 Al(NO₃)₃ (aq) + 3 H₂ (g) .. When 0.143 g of Al were added to 200 mL of 0.500 M HNO₃, 0.00842 g of H2 were produced. Find the percent yield of H₂.

(Please don’t forget to calculate the theoretical yield of hydrogen from both the aluminum and the nitric acid.)

A metal salt with the formula MCl2 crystallizes from water to form a solid with the composition MCl2⋅6H2O. The equilibrium vapor pressure of water above this solid at 298 K is 22.0 mbar .

What is the value of ΔrG for the reaction MCl2⋅6H2O(s)⇌MCl2(s)+6H2O(g) when the pressure of water vapour is 22.0 mbar ?

What is the value of ΔrG ∘ when the pressure of water vapour is 1 bar?

A buffer is prepared by mixing 25.0 mL of 0.500 M NH₃(aq) with 25.0 mL of 0.200 M HCl (aq). What is the pH of the buffer? [ K_b (NH₃) = 1.8 x 10^-5 ]

A 37.00 mL solution of 0.390 M weak acid Ha(aq) (Ka=2.25x10^-5) is titrate with 0.390 M NaOH(aq). Calculate the pH of the solution 14.00 mL past the end point.

1. Find the number of moles that are in 2.93g of LiO2 and report it with the correct number of significant figures
a. 8.75 x 10^22 mol
b. 9.81 x 10^-2 mol
c. 0.0980589 mol
d. 87.5 mol

2. calculate the mass of Chromium (Cr) in magnesium dichromate (MgCr2 O7)
a. 21.6%
b. 23.1%
c. 43.3%

3. A gold wedding band contains 2.3 x 10^22 Au atoms. How many moles of gold are in the wedding band?
a. 3.8 x 10^-2 mol Au
b. 26.2 mol Au
c. 3.8 mol Au
d. 3. 92 mol Au

110mg CaCl2 and 50mg CaSO4 added to 500mL water. solution pH is 8.0 ([H+]=10E-8M ; [OH-]= 10E-6 M). assuming all salts dissociate completely express concentrstion of Ca2+, Cl-, SO42- in mg/L, millimolar, normal (N) units. if total molar concentrations of all speicies in solution is same as in pure water, what are mole fractions of H+, OH-, Ca2+, Cl-, SO42-, H2O

complete and balance the reaction shown assuming 100% neutralization

AL(OH)3 + H2C2O4=? SHOW WORK.

Two 20.0-g ice cubes at –15.0 °C are placed into 255 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.

I am posting this problem because I've had trouble following the steps listed in similar problems. Please don't answer if you are only going to copy/paste a version of those same steps; It will not be helpful.

When a suspected drunk driver blows 186 mL of his breath through this breathalyzer, the breathalyzer produces an average of 323 mA of current for 10 s. Assuming a pressure of 1.0 atm and a temperature of 24 ∘C, what percent (by volume) of the driver's breath is ethanol?