| Net Ionic Equations | Electrolytes & Solubility | Calorimetry | Thermochemistry misc. | Gas Laws |
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What is Spectator ions?
An ion that exists as both a reactant and product in the total ionic equation.
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What is electricity?
Electrolytes are substances that, when dissolved in water, conduct _____.
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What is 1 Joule?
1 Kg * m^2*s^-1 is equal to ___________.
(' * ' indicates multiplication & '^' indicates superscript/charge) |
What is -16 J?
U = q + w = (+125 J) + (-141J) = -16 J
Calculate the overall change in internal energy for a system that absorbs 125 J of heat and does 141 J of work on the surroundings.
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What is decreases?
As the volume of a gas increases, the pressure decreases. The volume of a given amount of gas held at constant temperature is inversely proportional to its pressure. This can be seen in P1V1=P2V2.
As the volume of a gas increases, the pressure __________.
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What is 2 NaI + 1 Ag2S ?
(numbers separated with a space indicate coefficients; numbers NOT separated with space indicate subscript/quantity of elements)
Predict the products of the following chemical equation:
1 Na2S + 2 AgI → |
What is precipitates?
Solids formed from a insoluble reaction are called _____.
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What is 4.184 J/g℃
(4.184 Joules per grams*degrees Celsius)
What is the specific heat of H2O?
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What is 24.4 atm?
(1 atm=760 torr) (P1V1)/T1=(P2V2)/T2 (0.925 atm)(25.2 L)(273K)/(298K)(.875atm) = 24.4 atm
The volume of a gas is 25.2 liters at 25.0 degrees Celsius and 0.925 atm of pressure. What is the volume if the temperature decreases to 0.00 degress Celsius and the pressure decreases to 665 torr?
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What is 4.15 g of CO?
Calculate the mass of 5.62 L of CO gas measured at 80ºC and 580 mmHg.
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What is H^+(aq) + Cl^−(aq) + Na^+(aq) + OH^−(aq) → Na^+(aq) + Cl^−(aq) +H2O(l)
('^' indicates superscript i.e. charge)
Predict the Total Ionic Equation of the following chemical equation:
HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) |
What is Cloudiness/Haziness and/or solid if enough precipitate is formed?
What visible sign(s) show that a precipitate was formed?
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What is 0.162 Jg*℃?
0= q(H2O) + q(metal) -q(metal) = q(H2O) -(350 g) (c) (28.57 ℃ - 95℃) = (250 g) (4.184J/g*℃ ) (28.57℃ - 25℃) -(350 g) (c) (-66.43℃) = 1056 (3.57℃)) 23,250.5 (c) =3,769.92 C = 0.162 J/g*℃
350 grams of metal is placed at 95℃ was placed in 250g of water at 25 ℃, the final temperature was 28.57 ℃. What is the specific heat of the metal?
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What is -890.3 kJ/mol or 890.3 kJ/mol released?
Hrxn = nHf (products) - mHf (reactants) = [1(393.5) + 2(285.8)] [1(74.8) + 2(0)] = 890.3 kJ/mol released (exothermic) or -890.3 kJ/mol
Calculate the H rxn for the following reaction from the table of standard values.
CH4 (g) + 2O2 (g) -> CO2 (g) + 2H2O(l) CH4 △H= -74.6 kJ/mol CO2 △H= -393.5 kJ/mol H2O △H= -285.8 kJ/mol |
What is 8612.2mL?
A sample of a gas occupies 9.80x103 mL at 25ºC and 870 mmHg. What volume will it occupy at the same temperature and 990 mmHg?
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What is 3 Cu^2+(aq) + 2(PO4)^3-(aq) -> Cu3(PO4)2 (s)
('^' indicates superscript i.e. charge) (numbers separated with a space indicate coefficients; numbers NOT separated with space indicate subscript/quantity of elements)
Predict the Net Ionic Equation of the following chemical equation:
3 CuCl2(aq) + 2 K3(PO4)(aq) -> 6 KCl(aq) + 1 Cu3(PO4)2(s) (numbers separated with a space indicate coefficients; numbers NOT separated with space indicate subscript/quantity of elements) |
What is Ca3(PO4)2 (s) or Calcium Phosphate?
What insoluble product, if any, occur from the following: Na3PO4 (aq) + CaCl2 (aq) ?
(numbers not separated with space indicate subscript/quantity of elements) Rules: 1.Compounds of group 1 elements (Li+, Na+, K+, Rb+, Cs+, and Fr+) and ammonium (NH4+) are soluble. 2.Nitrates (NO3–), chlorates (ClO3–), perchlorates (ClO4–), and acetates (C2H3O2–) are soluble. 3.Chlorides (Cl–), bromides (Br–), and iodides (I–) are soluble, except for those of Ag+, Pb2+, and Hg22+. 4.Except for compounds of the cations in guideline 1, carbonates (CO32–), sulfites (SO32–), phosphates (PO43–), and chromates (CrO42–) are insoluble. |
What is delta H = 57 kJ/ mol?
Q = mc△T Q= (200 g) (4.184Jg*℃)(6.8 ℃) Q =5,690 J = 5,700 J = 5.70 kJ Delta H= (5.70 kJ)/(1.00 M H2O /0.100 L of H2O) Delta H = 57 kJ/ mol
100. mL of 100. M NaOH is mixed with 100 mL of 1.00 M HCl inside a coffee cup calorimeter. Both solutions were initially at 21.1℃, and after the reaction was complete the calorimeter measured the temperature as 27.9 ℃. What is the enthalpy of the reaction?
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What is △H= -283.0kJ/mol?
=-393.5 kJ/mol - (-110.5 kJ/mol)= -283.0 kJ/mol
Given the following reactions and enthalpies..
C + 1/2 O2 -> CO △H=-110/5 kJ/mol C + O2 ---> CO2 △H= -393.5 kJ/mol ----------------------------------------------------- CO + 1/2 O2 → CO2 △H= ? Calculate △H for the target equation. |
What is 104.4 mL?
A syringe containing 87.0 mL of air is at 400 K. What will the volume of the syringe be if it is placed in a boiling water bath (480 K). Assume pressure and the number of particles are held constant. Find the volume at 480 K.
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What is H^+(aq) + OH^–(aq) → H2O(l)
('^' indicates superscript i.e. charge)
Predict the Net Ionic Equation of the following chemical equation: HCl(aq) + KOH(aq) → KCl(aq) + H2O(l)
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What are HCl, HBr, HI, HNO3, HClO3, HClO4, and H2SO4?
(numbers not separated with space indicate subscript/quantity of elements)
Name the strong acid electrolytes.
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What is -2229.46 kJ/mol propanol?
qv=-CcalΔT qv=−810.1 J/℃ (95.8−50.0)℃ qV=-37102 J =−37.102 kJ 1.000 g propanol ( 1 mol60.09 g )= 0.016642 mol propanol ΔUrxn=qv=(−37.102 kJ)/(0.016642 mol propanol) ΔUrxn=1v=-2229.46 kJ/mol propanol
A 1.000 g sample of propanol, C3H7OH, is ignited inside a bomb calorimeter. The temperature rises from 50.0°C to 95.8°C. Given that the heat capacity of the calorimeter is 810.1 J/°C, determine ΔUrxn for the combustion of decane in units of kJ/mol of propanol .
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What is △Hrxn=14.36kJ?
H3BO3 (aq) → HBO2(aq) + H2O(l) △Hrxn = -0.02 kJ
H2B4O7(aq) + H2O(l) → 4 HBO2(aq) △Hrxn = -11.3 kJ H2B4O7(aq) → 2 B2O3(s) + H2O(l) △Hrxn = 17.5 kJ Using the above information, calculate △H of 2H3BO3(aq) → B2O3(s) + 3H2O(l). |
What is 395K?
A sample of oxygen has a pressure of 5.00×102 kPa at 40.00∘C. What will be the temperature in Kelvin at a pressure of 6.30×102 kPa?
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