10.0g of Fe(s) at 98.0 degrees Celsius is placed in 50.0mL of H2O(l) at 20 degrees Celsius. Assuming no energy is lost to the surroundings what is the final temperature of Fe(s) and H2O(l) at thermal equilibrium?
A) UO2<+2> b) As2O3 c) NaBiO3 d) As4 e)P4O6 f) Mg2P2O7 g) Na2S2O3 h) Hg2Cl2 i) Ca(NO3)2
1) AgNO3 + NaBr = 2) BaI2 + ZnSO4 = 3) Na2CO3 + MgCl(Chlorine)2 = 4) KOH + H3PO4 = 5) HCl + Fe(OH)3 =
Balance using the half reaction method in an acidic solution: Cr(NCS)6<4->(aq) + Ce<4+> (aq) = Cr<3+>(aq) + Ce<3+> (aq) + NO3<->(aq) + CO2 (g) + SO4<2->(aq)
Using the reaction of hydrogen chloride (hydrochloric acid) and calcium hydroxide to produce water and calcium chloride answer the following: A. How many moles of hydrochloric acid react with 0.5 moles of calcium hydroxide? B. How many grams of hydrochloric acid react with 1 mole of calcium hydroxide? C. How many grams of cal
Cyclopropane is used as a general anesthetic. If a sample of cyclopropane stored in a 2.00L container at 10.0 atm and 25C is transferred to a 5.00L container at 5.00 atm, what is the resulting temperature?
Using the reaction of hydrogen chloride (hydrochloric acid) and calcium hydroxide to produce water and calcium chloride answer the following: What is the maximum number of molecules of calcium chloride that can be formed in this reaction?
What is the net ionic equation of 2Fe(NH4)2(SO4)2*6H2O + 6K2C2O4 + H2O2 + H2SO4 2K3[Fe(C2O4)3]*3H20 + 3K2SO4 + 2(NH4)2 SO4 + 8H2O
2Fe(NH4)2(SO4)2*6H2O + 6K2C2O4 + H2O2 + H2SO4 ---- 2K3[Fe(C2O4)3]*3H2O + 3K2SO4 + 2(NH4)2SO4 + 8H2O I need to find the oxidation state of Iron in both the reagent side and product side of the equation.
A small smelter converts galena (lead sulfide) into pure lead by heating the ore with an excess of oxygen. Sulfur dioxide is produced as an air pollutant, as a result of the reaction. To remove sulfur dioxide, the flue gas is passed through a slurry of lime (calcium oxide) to produce calcium sulfate. The smelter processes 120
See attached for full problem. The concentration of isobutene in the overhead product is 4.8 mole %, and the concentration of propane in the bottoms is 0.7 mole %. Calculate the moles of the various components in the overhead and bottoms per 100 moles of feed.
What is the consequence (what does it mean?) when a system has zero degrees of freedom as calculated by the Gibbs Phase Rule? What do I need to conclude about such a system?
I am preparing for my chemistry exam and would appreciate a multiple choise quiz on the last chapter (i.e., ideal gas law, superconductivity, extensive properties, critical pressure, aerobic, etc.). Can you provide me with such a quiz with the answers provided. Thanks. Chemistry Quiz 2: Multiple Choice Questions 1) Eleme
A furnace burns a fuel oil, the composition of which can be represented as (CH2) n. It is planned to burn this fuel with 10 % excess air. Assuming complete combustion, calculate the composition of the flue gas on a dry basis. Please see attachment for the rest of the problem, including relevant diagrams.
The molecular weight of NaOH is 40. the molecular weight of a widely used buffer, HEPES, is 255. HEPES has a pK of 7.5 and is available in the acid form. how many grams og HEPES and NaOH are needed to produce one liter of a 0.5 molar solution of pH 7.5? of pH 7.0? of pH 8.5?
Balance the following reaction: Mn + HCl --> MnCl2 + H2 If you have 100g of Mn and 100g of HCl find a. The limiting reageant b. Moles of MnCl2 formed c. Grams of MnCl2 formed d. Moles of excess reagent
If Aluminum Chloride reacts with Copper II Carbonate and 0.25 moles of Aluminum Chloride are used, how much Copper II Chloride is made in moles?
The sublimation pressures of solid chlorine are 352 Pa at -112 C and 35 Pa at -126.5 C. The vapor pressures of liquid Chlorine are 1590 Pa at -100 C and 7830 Pa at -80C. Calculate a)heat of vaporization b)heat of sublimation c)heat of fusio d)triple point I have already figured out the first three. The heat of sublimation
I have attached the graphs. I don't think the first one is useful, but i needed to plot the data and find the heat of vaporization. Hence, the reason for the second graph. I know that the slope is equal to the heat of vaporization/RT but I don't think I am getting the right answer.
Estimate the fugacity of nitrogen gas at 50 bar and 298 K.
2. Given the vibrational temperature of HCl is 4227 K, a) what is qvib at a temperature of 2600 K, keeping the zero point energy? and referenced to v = 0? b) what is qvib at a temperature of 3100 K, keeping the zero point energy and referenced to v= 0? c) What is the vibrational contribution to CV, at the temperature 2600 K
1. Given the rotational temperature of HCl is 15.02 K, a) what is the ratio of the number of particles in the J= 14 to the J=4 level at a temperature of 1900 K? b) What J level has the highest proportion of particles at the temperature 1900 K? c) What is the energy, E, of rotation at this temperature? d) What is the entr
For O2(g) in a 200mL container at 1500K, calculate q(trans) and the thermal wavelength.
How many fluid mls would fit into a box measuring 3626mm in lenth, 1875mm in width and 1216mm in height?
Set up the equations to solve P air (torr) : P H2O (torr) : change of H vap: and lnP.