1. 5.00 g of urea, (NH2)2CO is dissolved in 250.0 mL of water(density = 1.00 g/mL)...
1. 5.00 g of urea, (NH2)2CO is dissolved in 250.0 mL of water(density = 1.00 g/mL) at 30.0oC in a coffee cup calorimeter. When this is done, 27.6 kJ of heat is absorbed. (5 points)
a) Is the solution process exothermic or endothermic?
c) What is qwater?
d) What is the final temperature of the solution(specific heat constant of water is 4.18 J/g.OC)?
Please show all the work!! thank you very much :)
Homework Answers
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1. 5.00 g of urea, (NH2)2CO is dissolved
in 250.0 mL of water(density = 1.00 g/mL)...
ma E of urea, (NHCO. is dissolved in 250.0 ml. of water id-1.00/mL.) 27,6 kJ of heat is absorbed at the final tempe...
ma E of urea, (NHCO. is dissolved in 250.0 ml. of water id-1.00/mL.) 27,6 kJ of heat is absorbed at the final temperature of 56.4°C. What is the initial temperature of water? 56,4-1.) -21.6=(250)(4.1845/9 to -
Urea, (NH2)2CO, which is widely used in fertilizers and plastics, is quite soluble in water. If...
Urea, (NH2)2CO, which is widely used in fertilizers and plastics, is quite soluble in water. If you dissolve 6.51 g of urea in 15.0 mL of water, what is the vapor pressure of the solution at 24 °C? Assume the density of water is 1.00 g/mL. The vapor pressure of water at 24 °C is 22.4 mmHg. mmHg
When 16.3 g KOH is dissolved in 94.3 g of water in a coffee-cup calorimeter, the...
When 16.3 g KOH is dissolved in 94.3 g of water in a coffee-cup calorimeter, the temperature rises from 18.9 °C to 30.16 °C. What is the enthalpy change per gram (in J/g) of KOH dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/g×K. Water has a density of 1.00 g/ml. Be sure to enter the correct sign (+/-). Enter to 1 decimal place.
1. A coffee cup calorimeter was used for the neutralization reaction of 100 mL of 1.00...
1. A coffee cup calorimeter was used for the neutralization reaction of 100 mL of 1.00 M hydrochloric acid with 100 mL of 1.20 M sodium hydroxide. The initial temperature was 22.88 °C and the final temperature was 29.39 °C. Calculate the calorimeter constant for the reaction. HCl (aq) + NaOH (aq) NaCl (aq) + H2O (∆H°rxn = -58.3 kJ/mol) 2. The same calorimeter was used for the dissolution of 8.86 g sample of lithium chloride in 100.0 mL of...
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of...
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee- cup calorimeter, the temperature of the resulting solution increases from 21.3°C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of Mgo. Assume that the specific heat capacity of the solution is 4.18 J/g.K, and the density of the solution is 1.00 g/mL. - 131 kJ O -613 kJ O-328 kJ 0 -28.3 kJ
3. In a dissolution experiment, 5.0 g of NH4NOs was dissolved in 50.0 mL of water...
3. In a dissolution experiment, 5.0 g of NH4NOs was dissolved in 50.0 mL of water in a calorimeter If the calculated for the reaction was 1.7 kJ, calculate the observed Ar for the experiment. (Ignore the heat capacity of the calorimeter, i.e., use Ceup, -0. Assume the specific heat capacity of the solution = 4.18 J/g。C and the density of the water-1.0 g/mL)
Consider the following reaction: Mg (s) + 2 HCl (aq) → MgCl2 (aq) + H2 (g)...
Consider the following reaction: Mg (s) + 2 HCl (aq) → MgCl2 (aq) + H2 (g) ΔHrxn = –4.6 × 102 kJ a. Is this reaction endothermic or exothermic? Circle one. [1] b. How much heat is evolved when 1.37 g of Mg are dissolved in excess HCl? [5] c. If 1.37 g of Mg are dissolved in enough HCl to make 250.0 mL of solution in a coffee-cup calorimeter, what is the final temperature of the solution? (Assume density...
When 4.102 g of KNO3 is dissolved in 39.825 g of water in a "coffee-cup calorimeter"...
When 4.102 g of KNO3 is dissolved in 39.825 g of water in a "coffee-cup calorimeter" at 24 degrees Celsius, the temperature of the solution went down to 19 degrees Celsius. a.) Is this solution reaction exothermic or endothermic? Why? b.) Calcualate qH2O using Eq. 1. c.) Find as it occured in the calorimeter (Eq. 4). d.) Find for the solution of one mole KNO3 in water. e.) Find for the solution of 1.00 g KNO3 in water.
8. A student conducts an experiment to determine the enthalpy of solution for lithium chloride dissolved...
8. A student conducts an experiment to determine the enthalpy of solution for lithium chloride dissolved in water. The student combines 5.00 grams of lithium chloride with 100.0 ml of distilled water. The initial temperature of the water is 23.0 °C and the highest temperature after mixing reaches 33.0 °C. Assume a density of 1.00 g.ml and a specific heat of 4.18 J/gºC. a. Is the reaction endothermic or exothermic? Justify your answer. b. Calculate the temperature change of the...
An 8.000 gram sample of solid NH.NO, was mixed with a 200.00 mL sample of water...
An 8.000 gram sample of solid NH.NO, was mixed with a 200.00 mL sample of water in a coffee cup calorimeter. The water was initially at 20.0°C and the final temperature of the resulting solution was recorded as 17.1°C. Calculate the experimental AHcoln (in units of kJ/mol NH.NO:) for the dissolution of NH NO3 (molar mass = 80.04 g/mol). Assume that no heat is lost to the calorimeter or the surroundings. The density of water is 1.00 g/mL and the...
ma E of urea, (NHCO. is dissolved in 250.0 ml. of water id-1.00/mL.) 27,6 kJ of heat is absorbed at the final temperature of 56.4°C. What is the initial temperature of water? 56,4-1.) -21.6=(250)(4.1845/9 to -
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee- cup calorimeter, the temperature of the resulting solution increases from 21.3°C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of Mgo. Assume that the specific heat capacity of the solution is 4.18 J/g.K, and the density of the solution is 1.00 g/mL. - 131 kJ O -613 kJ O-328 kJ 0 -28.3 kJ
3. In a dissolution experiment, 5.0 g of NH4NOs was dissolved in 50.0 mL of water in a calorimeter If the calculated for the reaction was 1.7 kJ, calculate the observed Ar for the experiment. (Ignore the heat capacity of the calorimeter, i.e., use Ceup, -0. Assume the specific heat capacity of the solution = 4.18 J/g。C and the density of the water-1.0 g/mL)
8. A student conducts an experiment to determine the enthalpy of solution for lithium chloride dissolved in water. The student combines 5.00 grams of lithium chloride with 100.0 ml of distilled water. The initial temperature of the water is 23.0 °C and the highest temperature after mixing reaches 33.0 °C. Assume a density of 1.00 g.ml and a specific heat of 4.18 J/gºC. a. Is the reaction endothermic or exothermic? Justify your answer. b. Calculate the temperature change of the...
An 8.000 gram sample of solid NH.NO, was mixed with a 200.00 mL sample of water in a coffee cup calorimeter. The water was initially at 20.0°C and the final temperature of the resulting solution was recorded as 17.1°C. Calculate the experimental AHcoln (in units of kJ/mol NH.NO:) for the dissolution of NH NO3 (molar mass = 80.04 g/mol). Assume that no heat is lost to the calorimeter or the surroundings. The density of water is 1.00 g/mL and the...
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