Consider a titration of 0.15M NaOH and 250 mL of 0.10M HBr.
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Part A.) Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g)+Cl2(g)⇌COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 475 ∘C . At equilibrium, the concentrations were measured and the following results obtained: Gas Partial Pressure (atm) CO 0.840 Cl2 1.28 COCl2 0.130. What is the equilibrium constant, Kp, of this reaction?
Part B.) The following reaction was performed in a sealed vessel at 797 ∘C :
H2(g)+I2(g)⇌2HI(g)
Initially, only H2 and I2 were present at concentrations of [H2]=3.00M and [I2]=2.35M. The equilibrium concentration of I2 is 0.0700 M . What is the equilibrium constant, Kc, for the reaction at this temperature?
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FOR QUESTION 5-7):Solve the problems completely
5) 1.60 g of an unknown molecular substance is dissolved in 20.0 g of benzene. The freezing point of pure benzene is 5.5oC, and the freezing point of the mixture is 2.8oC. What is the gram formula mass of the unknown substance?
6) Complete the following two Bronsted-Lowrey reactions and indicate the acid (A), base (B), conjugate acid (CA), and conjugate base (CB). (20)
HSO4-(aq) + H2O(l)
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Air is 21.0% by volume oxygen molecules and C3H8 produces CO2 and H2O on combustion. What volume of air at 1.00 bar and 20.0 °C would be required to burn 38.8 Kg of propane (C3H8)?
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When a 22.0 mL sample of a 0.448 M aqueous hydrocyanic acid solution is titrated with a 0.387 M aqueous barium hydroxide solution, what is the pH after 19.1 mL of barium hydroxide have been added? pH =
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Order these chemical species by increasing pH of an 0.1M aqueous solution of each. That is, imagine making an 0.1M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species relative pH of 0.1M aqueous solution HF ▼(Choose one) ClO2− ▼(Choose one) HClO2 1 (lowest) H2O 4 NO2− 7 OH− ▼(Choose one) F− 6 HNO2 ▼(Choose one)
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In the following reaction:
HCO3-(aq) + NH3(aq) ↔ CO32-(aq) + NH4+(aq)
Select one:
a. NH3 is an acid and HCO32- is its conjugate base.
b. NH3 is an acid and NH4+ is its conjugate base.
c. HCO3- is an acid and CO32- is its conjugate base.
d. NH4+ is an acid and CO32- is its conjugate base.
e. HCO3- is an acid and NH3(aq) is its conjugate base.
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Dimethylhydrazine is a carbon-hydrogen-nitrogen compound used in rocket fuels. When burned completely, a 0.312 g sample yields 0.458 g CO2 and 0.374 g H2O. What is the empirical formula of diemthylhydrazine?
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Write equations for the reaction of each substance in oxygen if a reaction occurs:
1. Adding glowing orange wooden splint to oxygen and it relighting.
2. Adding glowing orange steel wool to oxygen and it sparkling.
3. Adding glowing orange charcoal to oxygen and relit
4. Adding burnt sulfur to oxygen and it relighting with blue flame
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1)
Which of the following compounds exhibits optical isomerism?
Which of the following compounds exhibits optical isomerism?
| CH3-CHBr-CH3 | |||||||||||||||||||||
| CH3-CH2-CHF-CH3 | |||||||||||||||||||||
| CH3-CH2-CH3 | |||||||||||||||||||||
| CH3-CH2-CH2F | |||||||||||||||||||||
|
CH3-CH2-CBr2-CH3 2) Based on the molecular formula, determine whether each compound is an alkane, alkene, or alkyne. (Assume that the hydrocarbons are noncyclical and there is no more than one multiple bond.) Drag the appropriate items to their respective bins. "C3H6 C4H10 C4H6 C2H2" Alkane Alkene Alkyne 3) Which of the following alkane names is correct? Which of the following alkane names is correct?
|
5)
Write the balanced chemical equation for the catalytic hydrogenation (addition of H2) to CH3CH=CHCH3.
Write the balanced chemical equation for the catalytic hydrogenation (addition of H2) to CH3CH=CHCH3.
| CH3CH=CHCH3 + H2 → CH3CH2CH2CH3 | |
| CH3CH=CHCH3 + 2 H2 → 2 CH3CH3 | |
| CH3CH=CHCH3 + 3 H2 → CH3CH3 + 2 CH4 | |
| CH3CH=CHCH3 + 2 H2 → CH3CH2CH3 + CH4 | |
|
CH3CH=CHCH3 + 4 H2 → 4 CH4 |
6)
Write the balanced chemical equation for the addition of HBr to CH2=CHCH2CH3.
Write the balanced chemical equation for the addition of HBr to CH2=CHCH2CH3.
| CH2=CHCH2CH3 + 2 HBr → CH3Br + CH2BrCH2CH3 | |
| CH2=CHCH2CH3 + HBr → CH3CHBrCH2CH3 | |
| CH2=CHCH2CH3 + 4 HBr → 4 CH3Br | |
| CH2=CHCH2CH3 + 2 HBr → 2 CH2BrCH3 | |
8)
Which of the following names is correct?
Which of the following names is correct?
| 1,2,4-trifluorobenzene | |
| 2,5-dibromocyclohexene | |
| 4-isopropyl-6-methylbenzene | |
| 1,3,4-fluorobenzene | |
| 1-methyl-3-isopropylhexene |
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Write the dissociation reaction for the following acids in water. Use the appropriate arrow symbols. Label the acid, base , conjugate acid and conjugate base for each:
HCl(hydrochloic acid)
C6H6COOH (benzoic acid)
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What is the pH at the equivalence point in the titration of a 23.0 mL sample of a 0.304 M aqueous hydrocyanic acid solution with a 0.433 M aqueous sodium hydroxide solution?
pH =
A 30.6 mL sample of a 0.393 M aqueous acetic acid solution is titrated with a 0.296 M aqueous potassium hydroxide solution. What is the pH after 16.7 mL of base have been added?
pH =
When a 18.0 mL sample of a 0.476 M aqueous acetic acid solution is titrated with a 0.320 M aqueous potassium hydroxide solution, what is the pH after 40.2 mL of potassium hydroxide have been added?
pH =
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A 1 liter solution contains 0.436 M hypochlorous acid and 0.581 M sodium hypochlorite.
Addition of 0.109 moles of barium hydroxide will:
(Assume that the volume does not change upon the addition of barium hydroxide.)
Raise the pH slightly
Lower the pH slightly
Raise the pH by several units
Lower the pH by several units
Not change the pH
Exceed the buffer capacity
A 1 liter solution contains 0.460 M hydrofluoric acid and 0.345 M potassium fluoride.
Addition of 0.380 moles of hydrobromic acid will:
(Assume that the volume does not change upon the addition of hydrobromic acid.)
Raise the pH slightly
Lower the pH slightly
Raise the pH by several units
Lower the pH by several units
Not change the pH
Exceed the buffer capacity
A 1 liter solution contains 0.401 M hydrofluoric acid and 0.301 M potassium fluoride.
Addition of 0.150 moles of hydrobromic acid will:
(Assume that the volume does not change upon the addition of hydrobromic acid.)
Raise the pH slightly
Lower the pH slightly
Raise the pH by several units
Lower the pH by several units
Not change the pH
Exceed the buffer capacity
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How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.175 M NaOH solution?
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