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Final temperature after urea dissolves in water
Urea, (NH2)2 (CO), is used in the manufacture of resins and glues. When 5.00 g of urea is dissolved in 250.0 mL of water (d=1.00 g/mL) at 30.0°C, 27.6 kJ of heat is absorbed. What is the final temperature of the solution in kJ? The density of water is 4.18 J/g·°C. What is the final temperature in °F? F = °C x 1.8 + 32 (Round your answer to one decimal place)
Determine the mass percentage concentration of a sodium hydroxide solution produced by mixing 50.0 mL of a 25 % (density=2.45g/mL) sodium hydroxide solution with 10.0mL of H 2 O?
Determine what type of bond is expected for a compound formed between Magnesium and Oxygen Based on these values,?
Determine what volume of 1.0 mol/L solution of Copper monosulfide can be made from 23.9 grams of Copper monosulfide?
An equilibrium mixture at 225 degrees C contains 0.10 M NH3 and 0.20 M H2 for the reaction 3H2 (g) + N2 (g) --- 2NH3(g) If the Kc at this temperature is 1.7 X 10 2.
a sample of gas occupoes 17ml at -112 degrees C. what volume does the sample occupy at 70 degrees C.
If you a litre (1000mL) bottle of oil in your engine, how much heat is produced in kcal?In BTU To solve this problem you must know the density of motor oil is .82 g/mL.
A gas occupies a volume of 2.45 L at a pressure of 1.03 atm. What volume will the gas occupy as the pressure changes to 0.980 atm.
Considering given equation as P4(s) + 5 O2(g) P4O10(s) where ΔH = -3013 kJ/mol you just need to compute the heat evolved when 436 grams of white Phosphorous (P4)burns in air according to the given equation as above.
A sample of 6.022 g of CH4 is enclosed in a 12 L container at 402 K. What is its pressure in atmospheres
This assignment inhibits chemistry Laboratory Questions.
Calculate the solubility of Ni(OH)2 in a) distilled water and b) at pH of 4.0. Justify your answer. I know I need to use a mass balance ans the reaction for disolution is
The latent heat of vaporization of water is 577 J/kg. If a person's body needs to lose 345 J of energy through sweating, how many kilograms of water in the form of sweat must be evaporated.
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