(a)
Interpretation:
The symbol
Concept introduction:
For any substance in the mixture, mole fraction is equal to the ratio of number of moles of that substance in total moles of the mixture.
(b)
Interpretation:
The symbol
Concept introduction:
The partial pressure of pure solvent is defined as ratio of partial pressure of solvent in the presence of solute to the mole fraction of the solvent.
(c)
Interpretation:
The symbol
Concept introduction:
Freezing point is defined as the temperature showing equilibrium between solid and liquid solvent. At this point, the vapor pressure of both is same.
(d)
Interpretation:
The symbol
Concept introduction:
The Van’t Hoff factor is defined as a measure of solute’s effect on the colligative properties of the solution.
(e)
Interpretation:
The term activity needs to be explained.
Concept introduction:
In
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GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
- The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forwardA soft drink contains an unknown mass of citric acid, C3H5O(COOH)3. It requires 6.42 mL of 9.580 × 10−2-M NaOH to neutralize the citric acid in 10.0 mL of the soft drink. C3H5O(COOH)3(aq) + 3 NaOH(aq) → Na3C3H5O(COO)3(aq) + 3 H2O(ℓ) Determine which step in these calculations for the mass of citric acid in 1 mL soft drink is incorrect? Why? n (NaOH) = (6.42 mL)(1L/1000 mL)(9.580 × 10−2 mol/L) n (citric acid) = (6.15 × 10−4 mol NaOH) × (3 mol citric acid/1 mol NaOH) m (citric acid in sample) = (1.85 × 10−3 mol citric acid) × (192.12 g/mol citric acid) m (citric acid in 1 mL soft drink) = (0.354 g citric acid)/(10 mL soft drink) Determine the correct result.arrow_forwardAssume that the radius of Earth is 6400 km, the crust is 50. km thick, the density of the crust is 3.5 g/cm3, and 25.7% of the crust is silicon by mass. Calculate the total mass of silicon in the crust of Earth.arrow_forward
- A geochemist measures the concentration of sait dissolved in Lake Parsons and finds a concentration of 6.9 g-L. The geochemist also measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 2.7 gL. Assuming the salt concentration in Lake Parsons before it became isolated was equal to the average salt concentration in nearby non-isolated lakes, calculate the percentage of Lake Parsons which has evaporated since it became isolated. Round each of your answers to 2 significant digits.arrow_forwardA geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 69.32 g.L The geochemist also measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 5.02 g⋅L¯¹. Assuming the salt concentration in Lake Parsons before it became isolated was equal to the average salt concentration in nearby non-isolated lakes, calculate the percentage of Lake Parsons which has evaporated since it became isolated. Be sure your answer has the correct number of significant digits.arrow_forwardInsoluble Li2CO3 (s) precipitates when solutions of Na₂CO3(aq) and LiCl(aq) are mixed. Na2CO3(aq) + 2 LiCl(aq) → Li₂CO3 (s) + 2 NaCl(aq) A,HⓇ = ? To measure the enthalpy change, 100. mL of 0.65 M Na₂CO3(aq) and 100. mL of 1.3 M LiCl(aq) are mixed in a coffee-cup calorimeter. The temperature of the mixture rises by 1.3 °C. Calculate the enthalpy change for the precipitation of Li2 CO3(s) in kJ/mol. (Assume the density of the solution is 1.0 g/mL, and its specific heat capacity is 4.2 J/g. K.) kJ/mol Li₂CO3 A, H = =arrow_forward
- 1. Write an equation showing how the mass of the substance sought can be converted to the mass of the weighed substance on the right.arrow_forwardPhenobarbital was introduced in 1912 for the treatment of epilepsy. It is an anti-convulsant and sedative-hypnotic drug and used to control seizures. The measurement of phenobarbital is by fluorescence method. A 5.00 mL aliquots of an unknown containing phenobarbital were delivered to 50.00 mL volumetric flasks. The following volumes of a standard solution of phenobarbital, 2.00ug/mL, were then introduced to the volumetric flasks before diluting to volume with the corresponding signals on a fluorometer equipment. Find the concentration of phenobarbital in the original unknown sample.arrow_forwardEarth’s oceans have an average depth of 3800 m, a total surface area of 3.63x108 km2, and an average concentration of dissolved gold of 5.8x10-9 g/L. (a) How many grams of gold are in the oceans? (b) How many cubic meters of gold are in the oceans? (c) Assuming the price of gold is $1595/troy oz, what is the value of gold in the oceans (1 troy oz 5 31.1 g; d of gold 5 19.3 g/cm3)?arrow_forward
- Enter a balanced equation for the neutralization of each of the following. Part A H,SO, (aq) and KOH(aq) Express your answer as a chemical equation. Identify all of the phases in your answer. DA chemical reaction does not occur for this question Phases (states) should be entered in lowercase. No credit lost Try again Submit Previous Annweta Beaust Anawerarrow_forwardA newspaper article about the danger of global warming from the accumulation of greenhouse gases such as carbon dioxide states that "reducing driving your car by 20.0 miles a week would prevent release of over 1000. pounds of CO₂ per year into the atmosphere." To decide if this is a reasonable statement, calculate the reduction in the number of pounds of CO₂ a car would release in a year if its use was decreased by 20.0 miles per week. Think about the effects of possible variations in gas mileage on your answer. Gasoline is a complex mixture of hydrocarbons. In your calculations, assume that gasoline is octane (molecular formula C8H₁8) and that it is burned completely to CO₂ and H₂O in the engine of your car. Also assume that the car averages 26.4 miles per gallon and that the density of octane is 0.703 g cm-3. Reduction in pounds of CO₂ released = lbarrow_forwardo i MeO XS HCI 3. 40° C A A A 1. Br₂ 2. 2x t-Buo K* CN A CN CNarrow_forward
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