Calculate the change in internal energy (ΔE) for a system that is giving off 3.0 kcal of heat and is changing from 1.00 L to 8.00 L in volume at a pressure of 2.00 atm. (Remember that 101.3 J = 1 L∙atm; 1 cal = 4.18 J)

In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.0 rnL of 1.00 M HCI are mixed. Both solutions were originally at 24.6 °C. After the reaction, the final temperature is 31.3 °C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87 J/g-°C, calculate the ΔHneut/mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.

A 5.1-gram piece of gold jewelry isremoved from water at 100.0°C and placed in a coffee-cup calorimeter containing 16.9 gof water at 22.5°C (specific heat of water is 4.184 J/g · °C). The equilibrium (final)temperature of the water and jewelry is 23.2°C. The calorimeter constant is known fromcalibration experiments to be 1.54 J/°C. What is the specific heat (in J/g · °C) of this pieceof jewelry? If the tabulated value of the specific heat of gold is 0.129oC, is the jewelrypure gold?

A chemist measures the enthalpy change AH during the following reaction: 2 Al(OH),(s)-Al,0,(s) + 3H,0(1) AH=41. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ 3AI,0,(s) + 9H,0() 6Al(OH),(s) Al,0,(s) + 3H,0() 2Al (OH), (s) Al(OH),(6) - Al,0,(0) + ,00 1 Al,0,(5) + H,0() O kJ Explanation Check 2021 McGra M B

In a constant‑pressure calorimeter, 60.0 mL of 0.320 M Ba(OH)2 was added to 60.0 mL of 0.640 M HCl.The reaction caused the temperature of the solution to rise from 24.50 ∘C to 28.86 ∘C. If the solution has the same density and specific heat as water (1.00 g/mLand 4.184J/g⋅°C, respectively), what is ΔH for this reaction (per mole H2O produced)? Assume that the total volume is the sum of the individual volumes. ΔH= _________ kJ/mol H2O

When a 6.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 3.74 kJ · K¯¹, the temperature decreases by 0.400 K. Calculate the molar heat of solution of KSCN. ΔΗsoln = kJ/mol

A 47.70 mL volume of 1.00 M HCl was mixed with 47.30 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 25.0 J/°C) at 21.71 °C. The final temperature of the aqueous solution after the reaction was 29.73 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following:  The enthalpy change (∆H) for the neutralization in kJ/mol HCl ( this should be a negative number) in kJ/mol HCl