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 3Al,0,(s) + 9H,0(1) 6AI(OH), (s) ? Al,0,(s) + 3H,0() 2A1 (OH), (s) AI(OH),6) - A,0,0) + ,00) 1 ZAl,0,(s) + H,0(1)

Using the equations 2 H: (g) + O2 (g) → 2 H2O (I) AH° = -572 kJ/mol Ca (s) + ½ O2 (g) → CaO (s) AH° = -635 kJ/mol CaO (s) + H:O (1) → Ca(OH): (s) AH° = -64 kJ/mol Determine the enthalpy (in kJ/mol) for the reaction Ca (s) + 2 H2O (1) → Ca(OH)2 (s) + H2 (g).

In a coffee-cup calorimeter, 110.0 mL of 1.3 M and 110.0 mL of 1.3 M are mixed. Both solutions were originally at 22.2°C. After the reaction, the final temperature is 30.9°C. Assuming that all the solutions have a density of 1.0 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.

i need help with this question

3. 50.0 mL of 1.0 M sodium hydroxide and 50.0 mL of 1.0 M hydrochloric acid, both at 22.5 °C, were mixed together in a calorimeter. The temperature increased to 29.2 °C. Determine enthalpy of the reaction. You may assume that both solutions have the same density and heat capacity of water (d = 1.00 g/mL, SH=4.184 J/g°C). Remember, AH = q at constant pressure.

In a coffee-cup calorimeter, 110.0 mL of 1.4 M NaOH and 110.0 mL of 1.4 M HCl are mixed. Both solutions were originally at 24.0°C. After the reaction, 3 the final temperature is 33.4°C. Assuming that all the solutions have a density of 1.0 g/ cm° and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ - kJ/mol

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.19 kg sample of C,H,N from -4.5 °C to 6.6 °C. The experiment shows that 6.14 × 10° J of heat are needed. What can the chemist report for the molar heat capacity of C,H,N? Round your answer to 2 significant digits. O J-mol -1 - 1 ·K х10 ?

Section 5.6 You place 0.0750 g of magnesium chips in a coffee-cup calorimeter and then add 100.0 mL of 1.00 M HCI. The reaction that occurs is: -> Mg (s) + 2 HCI (aq) → H2 (g) + MgCl2 (aq) The temperature of the solution raises from 20.15 °C to 23.29 °C. What is the enthalpy change or the reaction per mole of Mg? Assume that the specific heat capacity of the solution is 4.20 J/g K and the density of the solution is 1.00 g/mL. 412 kJ/mol 428 kJ/mol -412 kJ/mol -428 kJ/mol

A chemist wastes a delicious brownie by burning it in a bomb calorimeter.  Before burning, the brownie weighed 18.19 grams. During the combustion process in the bomb calorimeter, the heat of the calorimeter increased by 8.75 ∘C.   The known heat capacity of the calorimeter that was used was 33.53 kJ/∘C.    What is the energy content, in kJ/g, of this brownie? Enter your answer with no units.

Calcium hydroxide is prepared by adding calcium oxide to water: CaO (s) + H2O (l) → Ca(OH)2 (s) Calculate the enthalpy change (ΔH) for this reaction considering the following experiment.  A 10.0 g sample of CaO (s) {MM = 56.08 g/mol} is added to 1.00 liter of water in a calorimeter with a total heat capacity of 4.37 kJ K-1 and the temperature increases by 2.70 K.