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Heat realsed by combustion of ethyl ether1. In earlier times, ethyl ether was commonly used as an anesthetic. It is, however, highly flammable. When 5.0 mL of ethyl ether C4H10 (l), (d=0.714 g/mL) is burned in a bomb calorimeter, the temperature rises from 23.5°C to 39.7. The calorimeter heat capacity is 10.24 kJ/°C. What is heat released when 5.00 mL ethyl ether is burned? (Round your answer to the nearest whole number)
2. The specific heat of aluminum is 0.902 J/g?°C. How much heat is absorbed by an aluminum pie tin with a mass of 473 g to raise its temperature from room temperature (23°C) to oven temperature (375°F)? F = °C x 1.8 + 32 (Give your answer in kJ and round to the nearest tenths)
Determine the enthalpy change if The heat released when 24.9 grams of Potassium K reacts with excess H2O water is 124 kilo joules?
What is the importance of chemistry to agriculture, Write summary of total one page and include references as well.
How many milliliters of 0.200 M NaOH will be required to titrate 7 mL of 0.479 M H2SO4
Solving this question helps the student to understand what is happening in a chemical reaction and to balance the given equation.
What volume (in mL) of a 1.420M NaOH solution is required to titrate 25.0mL of 4.50M HCl solution.
Heated and allowed to expand against a constant pressure of 1.20 atm until its volume reaches twenty eight Litres. Now determine Which of the given data is correct?
a sample of a certain beverage contains 1.00g of tartaric acid, H2C4H4O6. The beverage is titrated with 0.100M NaOH, how many millimeters of base are required to neutralize the tartaric acid.
2H2S (g) + 3O2 (g) → 2H2O (g) + 2SO2 (g) If 3.50 g of H2S are used in the above reaction, what will be the theoretical yield of water in grams.
What will be the freezing point and boiling point of this aqueous solution if given that Kb(H 2 O) = 0.51 oC/m and Kf = 1.86o C/m.
Compute KP at this temperature If the pH of an aqueous solution is 8.23, what are the hydrogen- and hydroxide-ion concentrations of this solution?
A 952 cm3 container of gas is exerting a pressure of 108 kPa while at a temperature of 48 oC. Calculate the pressure of this same amount of gas in a 1236 cm3 container at a temperature of 64 oC
CO(g) + 2H2(g) = CH3OH(g) , what is the equilibrium constant? , where CH3OH = 0.0412 atm, H2 = 0.274 atm, CO = 0.914 atm.
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