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How many kilojoules of heat are required to evaporate 1 liter of water at 1 atm if the initial water temperature is 20 degrees Celcius?
what is the percent relative error? Please explain by showing work. Are these measurements more precise or more accurate? What is the purpose of repetition in measurements?
A 10.0 mL sample of sulfuric acid from an automobile battery requires 35.08 mL of 2.12 M sodium hydroxide solution for complete neutralization.
Compare the numbers you have just calculated with the vapour pressures of water at these temperatures. Can you suggest a reason why the two sets of numbers are so different?
Consider one kmol of methane at a pressure of 23.2 bar and a temperature of 200 K. Is this methane an ideal gas? Show or describe how you reached this conclusion
Consider: C7H16 (l) + 11 O2 (g) → 7 CO2 (g) + 8 H2O (l) ΔH°reaction=- 4130 kJ. How much energy is released when 4.000 moles of C7H16, is combusted?
solution is diluted to a total volume of 278 mL. A 139-mL portion of that solution is diluted by adding 155 mL of water. What is the final concentration?
Calculate the osmotic pressure of a solution containing 18.55 of hemoglobin in 13.7 of solution at 24. The molar mass of hemoglobin is .
ICE Problem: Calculate Final Concentrations, Phosgene, COCl2 (g), is an extremely toxic gas. It was used during World War I. Today it is used to manufacture pesticides, pharmaceuticals, dyes, and polymers. It is prepared by mixing carbon monoxide ..
If 10500 L H2 gas is reacted with an excess of N2 gas at 200 atm. and 500 C, how many moles of ammonia gas would be produced, assuming a 15% yield?
A nugget of pure gold of 4.90 grams absorbed heat of 270 Joules. determine the final temperature of the Au if the initial temperature = 22.0°C? specific heat of Au =0.129 J/(g·°C).
An aqueous solution of Na2CO3 has a pH of 10.00. The CO3-2 (carbonate anion) is the conjugate base of its conjugate acid, HCO3- (bicarbonate anion). Write the net ionic equation for the reaction which shows why the solution has a basic pH.
The few gas analysis shows as carbon dioxide 14%, carbon monoxide 0.4%, oxygen 5.6% and nitrogen 80%. The air used has a dew point of 50°F. The barometer shows 29.9 inches of mercury. Calculate the dew point of the stack gas.
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