A scientist measures the standard enthalpy change for the following reaction to be -901.8 k) : Fe,03(s) + 2 Al(s)Al,03(s) + 2 Fe(s) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of Al203(s) is kJ/mol.

A 6.78 g sample of methanol was combusted in a bomb calorimeter. The temperature of the calorimeter increased by 12.7 °C. If the molar mass of methanol is 32.04 g/mol, and the heat capacity of the calorimeter is 5,104 J/°C, what is the molar AE for this reaction, in kJ/mol? Do not report units in your answer. Report your answer to one decimal place and include the correct sign.

From the following data, C (graphite) + O₂(g) → CO₂(g) H₂(g) + —⁄- 02₂(g) → H₂O (1) CH₂(g) + 20₂(g) → CO₂(g) + 2H₂O (1) kJ ×10 Calculate the enthalpy change for the reaction below: C(graphite) + 2H₂(g) CH4 (g) Be sure your answer has the correct number of significant digits. X → ΔΗ° S rxn ΔΗ° = -285.8 rxn = -393.5 ΔΗ° = -890.4 rxn kJ mol kJ mol kJ mol

A chemist measures the enthalpy change AH during the following reaction: Fe(s) + 2 HCl(g) →FeCl₂(s) + H₂(g) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction AH=157. kJ FeCl₂ (s) + H₂(g) → Fe(s) + 2HC1 (g) 2Fe (s) + 4H C1 (g) 3 FeCl₂ (s) + 3H₂(g) 2FeCl₂ (s) + 2H₂(g) 3Fe (s) + 6HCl (g) ΔΗ [ kJ kJ kJ 0x x10 × Ś

10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C

A scientist measures the standard enthalpy change for the following reaction to be 216.8 kJ :CH4(g) + H2O(g)3H2(g) + CO(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(g) is  kJ/mol.

Hot water heaters often use natural gas (methane) to generate heat. Methane and oxygen react to form carbon monoxide according to the overall equation: 2CH4(g)+3O2(g) = 2CO(g)+4H2O(g) The enthalpy of formation for each compound are as follows: CH4: - 74.6 O2: 0 CO: - 110.5 H2O: - 285.8 Part A: calculate the overall enthalpy change of the reaction. Part B: A typical water heater contains 40.0 gallons of water. After a long vacation, you come home and turn your water heater from "vacation mode" to hot. How many moles of methane must be combusted to heat the water in your water heater from 30.0°C to 48.0°C? The density of water is 3.79 kg/gal, the specific heat capacity of water is 4.182 J/g°C, and the water heater has a heat capacity of 850.0 J/g°C.

A bomb calorimeter has a heat capacity of 6.067 kJ/°C. A sample of vitamin (C31H4602) has an internal energy (DE) = -2.278 X 104 kJ/mol. When 1.434 g of the vitamin sample are burned in oxygen in the calorimeter, determine the final temperature in °C if the initial temperature is 14.51 °C.

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.A student heats 62.45 grams of platinum to 99.18 °C and then drops it into a cup containing 84.71 grams of water at 23.23 °C. She measures the final temperature to be 25.02 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.66 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of platinum.

A scientist measures the standard enthalpy change for the following reaction to be 79.4 kJ:NH4Cl(aq)NH3(g) + HCl(aq)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of HCl(aq) is  kJ/mol.