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30.0 mL of water at 24.5 °C was mixed with 40.0 mL of water at 40.0 °C. If the specific heat of water is 4.184 J/g °C and no heat was absorbed by the calorimeter, then the final temperature is _____ °C. (Report to the proper number of significant digits)
one day you notice that the outside temperature increase by 16 degrees Fahrenheit between your early morning jog and your lunch at noon. what is the corresponding change in temperature in the Celsius and Kelvin scales?
If 3.60 mL of vinegar needs 45.0 mL of 0.135 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.50 qt sample of this vinegar?
A gas has a volume of 590 mL at a temperature of -55.0C. What volume will the gas occupy at 30.0C.
2.00 moles of a gas occupies 62.2 L at a par- ticular temperature and pressure. Its density is 0.900 g/L. What is the molar mass?
A certain mass of oxygen was collected over water when potassium chlorate was decomposed by heating. The volume of the oxygen sample collected was 870 mL at 40C and a barometric pressure of 755 torr.
Wastewater flow in a sewer can be estimated by adding a known amount of tracer such as salt solution and measuring the salt concentration upstream and downstream of the point of addition.
Gas tank holds 42kg of gasoline. When gasoline burns, 147kg og oxygen are consumed and carbon dioxide and water are produced. What is the total combined mass of carbon dioxide and water that is produced?
Consider the reaction NO + O3 → NO2 + O2 Which has a rate constant given by k = 1.8×10-12 e-1370/T cm3 molecules-1 s-1 .Use the following standard heats of formation.
A 1.00 g sample of an unknown acid required 17.0 mL of .650 M NaOH to neutralize. What is the molar mass of the unknown acid?
Calculate: A) mL of NaOH needed to reach the equivalence point B) pH of the solution before the addition of any NaOH C) pH of the solution after the addition of 15.0 mL of NaOH
A concentrated sulfuric acid solution is 65.0% H2SO4 by mass and has a density of 1.55 g/mL at 20°C. What is the mass of 8.00 L of the concentrated sulfuric acid solution?
A vinegar sample contained 5.20 % acetic acid. How may mL of 0.450 N sodium hydroxide would be required to titrate 25.00 mL of the vinegar sample
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