could someone please help me with the calculations. im very confused 2. The heat of solution...
solve the blanks Data and Calculations 1. AH (neutralization & dilution) of 10 M H:SO4 and 1.00 M NaOH Keain Data Trial 1 Trial 2 Initial temperature of 10 M H2SO (5.0 mL in a graduated eylinder) 23.2 23.8 C C Initial temperature of calorimeter (50.0 mL of 1.00 M NaOH 45.0 mL water) 22.8 °C 2 1.5 °C Final temperature of the mixed solutions in calorimeter (50 mL 1.00 M NaOH 45.0 mL water 5.0 mlL 10 M H2SO)...
im trying to solve for the remaining but im confused please help this is experiment 25 Calorimetry HNO B. Enthalpy (Heat) of Neutralization for an Acid-Base Reaction H Poting flendar HCI + NaOH uuemliojo Trial 1 Trial 2 1. Volume of acid (mL) 50 - 60 Site 2. Temperature of acid (C) ao 20" 3. Volume of NaOH (ml) 20 4. Temperature of NaOH (C) Trial 1 5. Exact molar concentration of NaOH (mOVL) 6. Maximum temperature from graph (°C)...
help with number 7 please! 3. Heat gained by solution (temp. increase x 100 g x 4.184 J/K-9) = 6.5°C x 100g *4.181/ 2,719. 6 5 4. Heat gained by calorimeter (temp. increase X heat capacity of calorimeter) = (0.5°C x 74.30J/o 482.95, – 3,202.55, 5. Total joules released by reaction (3) + (4)] = 6. Complete: CH3COOH + NaOH CH3C06 Na+H2O 7. The number of moles of H,0 produced in reaction of 50 mL 1.0 M CH3COOH and 50...
DATA ANALYSIS I. You conducted the following three reactions in this experiment Reaction I(AHN): An aqueous solution of sodium hydroxide reacts with an aqueous solution of hydrochloric acid, yielding water and an aqueous salt Reaction 2 (AHs): Solid sodium hydroxide reacts with water, yielding aqueous sodium hydroxide . Reaction 3 (AHR): An aqueous solution of hydrochloric acid reacts with solid sodiu Reaction 1 (AHN)HCl(aq)+ NaOH(aq) NaCl(aq) + H20() 2 (AHs) hydroxide, yielding water and an aqueous salt AH (kJ/mol) Balanced...
A coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 190.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 °C to 23.86 °C. Calculate the enthalpy of solution, AH coln, per mole...
A coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 110.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 C to 23.83 C. Calculate the enthalpy of solution, AH soln per mole...
A coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 175.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 °C to 23.63 "C. Calculate the enthalpy of solution, AH gola, per mole...
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...
Average 솨 Verify Hess's L Average ΔΗΝ + Average ΔΗs MR, calculated _ AN: To calculate AHR. calculated take the sum of Average ΔΗΝ and A 4. from question 3. Compare this value to AHR. experimental from question 3. J/mol J/mol -J/mol _ J/mol as compared to ΔHR, experimental- experimental ween ΔΗR, calculated and your measured value ofdHR using the following formula IAHR.calculated- AHR,experimental l AHR,experimental % error 6. Calculate the percent error between your experimental value of AHR and...
please help When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 0.85 g of CaCl2(s) are dissolved in 100.10 g of water, the temperature of the solution increases from 24.36 to 25.89 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be...