Complete and balance each of the following equations for combustion reactions.
Express your answer as a chemical equation. Identify all of the phases in your answer.
A. C4H6(g)+O2(g)?
B. C(s)+O2(g)?
C. CS2(s)+O2(g)?
D. CH4O(l)+O2(g)?
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1. Calculate the molar amount of KHP used to neutralize the NaOH solution.
2. Calculate the molar concentration of the NaOH solution that you prepared.
3. Compare the actual molarity of your NaOH solution with your goal of 0.10 M.
Equivalance point-25.3,
Measurements found in lab.
| Mass of NaOH needed=0.40g | |
| Mass of KHP needed=0.505g | |
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Consider three hydrocarbon compounds: ethane, CH3CH3; ethene, CH2CH2; and
ethyne, CHCH, in all of which the two carbon atoms are bonded to each other. Of the three, ethyne has the _____________ carbon-carbon bond.
A. longest and strongest B. shortest and weakest
C. shortest and strongest D. longest and weakest
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Molarity of standard NaOH solution: x/1 H 2/3 Unknown + 2/3 NaOH -> 2/3 H2O +Na 2/3 Acetate
| Vinegar: | Titration 1 | Titration 2 | Tirtration 3 |
| Initial V of Acid | .01 mL | 5.56 mL | 11.32 mL |
| Final V of Acid | 5.56 mL | 10.71 mL | 16.02 mL |
| Inital V of Base | .01 mL | 27.12 mL | 3.01 mL |
| Final V of Base | 22.23 mL | 44.71 mL | 24.90 mL |
Unknown Acid code and number of reactive hydrogens: H+3
| Unknown Acid | Titration 1 | Titration 2 (Error) | Titration 3 | Titration 4 |
| Mass of Acid | .1024 g | .1028g | .1021g | .1023g |
| Initial V of Base | 24.90 mL | 37.80 mL | 45.5 mL | 9.24 mL |
| Final V of Base | 37.80 mL | 45.5 mL | 9.24 mL | 17.80 mL |
10. Find the moles of base (NaOH) for each of your unknown acid titrations.
11. Find the balanced equation using the number of reactive hydrogens (call an acid with one reactive hydrogen HA, one with two reactive hydrogens H2A, and so on).
12. Find the moles of unknown acid for each of your three unknown acid solutions.
13. Use the mass of unknown acid and the moles of unknown acid to find the formula mass of your unknown acid for each of your three unknown acid titrations.
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Rank the relative acid strengths of the following compounds: H2O, H2S, and H2Se
___ > ___ > ___
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Leachate is produced when precipitation infiltrates a sanitary landfill,
contacts the waste material, and appears at the bottom of the stored waste. Assume 6.9 kg of
benzene
(C 6 H 6 ) were placed in the landfill and it is all dissolved in the 90,000 gallons of leachate produced
during 1 year. What is the benzene concentration in the leachate during this 1 year in (a) mg/L, (b)
ppb m and (c) moles/L?
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a)Calculate the equilibrium constant at 10 K for a reaction with ΔHo = 10 kJ and ΔSo = 100 J/K.
b) Calculate the equilibrium constant at 105 K for the thermodynamic data in the previous question.
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1000 m3 of moist air at 101 kPa and 25 °C with a dew point of 11 °C enters a process. The air leaves the process at 98 kPa with a dew point of 58 °C. Assume ideal gases.
(a) Draw and label a flowsheet for the process.
b) What is the mole fraction of water in the air entering the process? Leaving the process?
(c) How many moles of water are added to or removed from the 1000 m3 of moist air?
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I have had such a hard time figuring out this problem please show with detailed response! thank you
Consider the titration of a 23.0?mL sample of 0.175M CH3NH2 with 0.155M HBr. Determine each of the following.
1.the initial pH
2.the volume of added acid required to reach the equivalence point
3.the pH at 6.0mL of added acid
4.the pH at one-half of the equivalence point
5.the pH at the equivalence point
6.the pH after adding 6.0mL of acid beyond the equivalence point
In: Chemistry
A. Write the Ksp expression for the sparingly soluble compound silver phosphate, Ag3PO4. Ksp=?
B. Write the Ksp expression for the sparingly soluble compound barium phosphate, Ba3(PO4)2. Ksp=?
C. The solubility of PbF2 is measured and found to be 0.527 g/L. Use this information to calculate a Ksp value for lead fluoride. Ksp=?
D.The solubility of Ag2CO3 is measured and found to be 3.55E-2 g/L. Use this information to calculate a Ksp value for silver carbonate. ksp=?
In: Chemistry
Write the balanced chemical equation for ethanol C2H6O burning in air as a LEAN mixture if the reactant side of the reaction is C2H6O + ?(O2 + 3.76N2) ===> ? CO2 + H2O + ? ?????
NOTE: A LEAN mixture means you have more air than you need to burn all the fuel. You will have excess oxygen left over after the reaction process.
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Volumes and molarities for titration of CdC2O4 solutions.
PART A Data
Initial reading of buret (KMnO4) (mL) 0.50
Final Reading of buret (KMnO4) (mL) 14.00
Molarity of KMnO4 solution (M) 0.000969
PART B DATA
Initial Reading of buret (NH3) (mL) 1.00
Final reading reading of buret (NH3) mL 22.50
Molarity of NH3 solution (M) 5.00
FOR PART A Find:
Moles of MnO4- used for titration (mol)
Moles of C2O42- in 100.0mL of solution (mol)
Molarity of C2O42-(M)
Molarity of Cd2+ (M)
Ksp of CdC2O4
For PART B Find:
Total Moles of C2O42-
Molarity of C2O42- (M)
Total moles of Cd2+ (mol)
Moles of [Cd(NH3)4 2+] (mol)
Molarity of [Cd(NH3)4 2+] (M)
Moles of NH3 added by titration (mol)
Moles of NH3 that did not react with Cd2+ (mol)
Molarity of NH3 that did not react with Cd2+ (M)
Kf for [Cd(NH3)4 2+]
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Gold is isolated from rocks by reaction with aqueous cyanide, CN-: 4 Au(s) + 8NaCN(aq)+O2(g)+H20(l)-> 4Na[Au(CN)2](aq)+4NaOH(aq). (a)Which atoms from which compounds are being oxidized, and which atoms from which compounds are being reduced? (b) The[Au(CN)2]- ion can be converted back to Au(0) by reaction with Zn(s) powder. Write a balanced chemical equation for this reaction. (c) How many liters of a 0.200 M sodium cyanide solution would be needed to react with 40.0kg of rocks that contain 2.00% by mass of gold?
In: Chemistry
In: Chemistry
Draw a log modulus–temperature plot for an amorphous polymer. What are the five regions of viscoelasticity, and where do they fit? To which regions do the following belong at room temperature: chewing gum, rubber bands, Plexiglas®?
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