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If 7.3 kJ of energy are required to change the temperature of water from 5.0°C to...
How much energy is required to change the temperature of 1.50 L of water from 25.0 °C to 100.0 °C? The specific heat capacity of water is 4.184 J/g·°C; density H2O = 1.0 g/mL; 1000 mL = 1 L Which of the following pairs of aqueous solutions will react to produce a precipitate (an insoluble solid) when mixed together? Group of answer choices Li2CO3 and HClO4 Li2SO4 and SrCl2 NaCl and KBr NaOH and HCl
a. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g of liquid ethanol from -5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid= 2.46J/g°C AHvap=38.6 kJ/mol b. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g water from 5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid=4.184 /g°C AHvap=40.7 kJ/mol
18. How much energy is needed to change the temperature of 25.00 mL of water from 10.0°C to 95.0°C? (c 4.1 84 J/(g·°C), d = 1 .00 g/mL) a. 160 k b. 2,880 kJ c. 8.9 k d. 6.4 kJ c. 105 k
Calculate the amount of heat (in kJ) required to raise the temperature of 150.0mL of water from 22˚C to 50˚C. The specific heat of water is 4.184 J/g*˚C. q=msΔ
C-1 How much heat is required to raise the temperature of 2000 g of water from 50°C to 80°C? The specific heat of water is 4.184 J/g °C a) 110.46 kJ b) 169.45 kJ C ) 251.04 kJ d) 301.25 kJ C-2 An exothermic reaction causes the surroundings to a) warm up b) become acidic c) condense d ) decrease in temperature C-3 Which of the reactions below have a positive entropy change? a) PC13(g) + Cl2(g) PCIs(8) b) NH3(g)...
1.If 245 Joules is required to change the temperature of 14.4 g of Chromium by 38.0 K, What is the specific heat of capacity of Chromium? 2. Calculate the energy in the form of heat (in kJ) required to convert 225 grams of liquid water at 21.0 °C to steam at 115 °C. (Heat of fusion = 333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: liquid water = 4.184 J/g·K, steam = 1.92 J/g·K)
a6f34c2c2eb8&attempt 1 Question 1 Volume Water 114.64 mL Initial Temperature of Water 60 °C Volume of Compound Y 100 mL 25 Initial Temperature of Compound Y °C 36.08 °C Final temperature of Compound Y + Water Question 2 Calculate the specific heat of Compound Y from your data. The specific heat of water is 4.184 J/gºC and its density is 1.00 g/mL. The density of compound Y is 2.78 g/mL. J/g°C
1. A volume of water was heated to 81.76 °C and immediately added to 48.80 mL of water at 20.55 °C contained within a coffee cup calorimeter. The final temperature of the mixture was 37.73 °C. The final volume of water inside the calorimeter was 92.03 mL. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: a. The volume of hot water added ml b. The mass of hot water (dwater = 1.00 g/mL) g...
Calculate the amount of energy (in kJ) necessary to convert 557 g of liquid water from 0°C to water vapor at 172°C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g ·°C, and for steam is 1.99 J/g ·°C. (Assume that the specific heat values do not change over the range of temperatures in the problem.) = KJ
Calculate the amount of energy (in kJ) necessary to convert 557 g of liquid water from 0C to water vapor at 182C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g C, and for steam is 1.99 J/g C. (Assume that the specific heat values do not change over the range of temperatures in the problem.)