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An aqueous antifreeze solution is 48.5% ethylene glycol (C2H6O2) by mass. The density of the solution is 1.062 g/cm3. Calculate the molality, molarity and mole fraction of ethylene glycol
A graduated cylinder contains 129 mL of water. A 17.0 g piece of iron (density = 7.86 rm{g/cm^3}) and a 17.0 g piece of lead are added. What is the new water level in the cylinder?
What unusual aspect of water is responsible for it unique characteristics as both a liquid and as a solid? Give examples of how this property of water would affect food systems during processing.
calculate the micrograms (to the nearest microgram) of iodine per serving in the finished product. Show your work.
How much ethylene glycol (C2H6O2) the major component of antifreeze, must be added to 1 L of water to keep it from at -15 F? Kf= 1.86 C/m.
how many grams of KOH are present in 32.5mL of a 6.42 M KOH solution
Calculate the mass percent of carbon in the compound and calculate What is its final temperature
How much heat do you need to raise the temperature of 150 g of gasoline from 30oC to 15oC?
Detremine the volume of CO2 produced at the temperature of 23 degree celsius and pressure of 0.985atm?
Imagine that you have a 6.50L gas tank and a 2.50L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch.
Kp for the reaction of SO2(g) with O2 to produce SO3(g) is 3 × 1024 . Calculate Kc for this equilibrium at 25ºC. (The relevant reaction is 2SO2(g) + O2(g) 2SO3(g).)
A car battery contains 1.0 L of 4.3 M sulfuric acid. Using the value in your answer to question E., calculate how many TUMS® tablets would be required to neutralize all the sulfuric acid in a car battery.
The temperature of a sample of water increases from 21.9°C to 45.3°C as it absorbs 5669 J of heat. What is the mass of the sample.
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