Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl,(g) – 2 MCI, (s)

Measurements show that the energy of a mixture of gaseous reactants increases by 396. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 122. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. O exothermic Is the reaction exothermic or endothermic? O endothermic

The compound WO3(s) is utilized in the refining process of tungsten from its mineral ore. Tungsten can be produced as follows: Reaction 1: WO3(s) + 3H2(g) → W(s) + 3H2O(g) a) From the following data calculate the enthalpy of the above reaction Reaction 2: 2W(s) + 3O2(g) → 2WO3(s)          ΔH = –1685.4 kJ Reaction 3: 2H2(g) + O2(g) → 2H2O(g)            ΔH = –477.84 kJb) Estimate the change of internal energy for Reaction 1. c) Is Reaction 1 exothermic or endothermic?

A scientist measures the standard enthalpy change for the following reaction to be -138.9 kJ: H,(2) + C,H,(g)C,H(g) kJ/mol. Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of C,H (g) is

A generic solid, X, has a molar mass of 82.3 g/mol. In a constant-pressure calorimeter, 46.1 g of X is dissolved in 337 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 29.50 °C. Assume the solution has the same specific heat as water, 4.184 J/(g.°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? q = kJ What is the enthalpy of the reaction? AHrxn kJ/mol =

Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2 H40, by the reaction C2 H4O(g) + H,0(1) HOCH, CH,OH(!) Use Hess's law to obtain the enthalpy change for this reaction from the following enthalpy changes: 2C, HO(g) + 502(9) → 4CO2 (9) + 4H,0(1) AH =-2612.2 kJ HOCH, CH, OH(1) + O2 (9) → 2002 (9) + 3H,0(1) AH=-1189.8 kJ Enthalpy change = kJ %3D

When 2.232 g of AX (s) dissolves in 147.5 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 34.8 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX (s) → A*(aq) + X¯ (aq) Assumptions for this calculation: · The specific heat of the solution is the same as that of pure water (4.18 J/gK) • The density of water = 1.000 g/mL · The liquid's final volume is not changed by adding the solid · The calorimeter loses only a negligible quantity of heat. The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change. Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.

A chemist measures the enthalpy change AH during the following reaction: 4 Fe(s) + 3 02(g)→2 Fe,O3(s) AH =-320. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 Fe(s) + 0,6) - Fe,0,(1) O kJ 2Fe,0; (s) – 4Fe(s) + 30, (3) O kJ 4Fe,0, (s) - 8Fe(s) + 60, (3)

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.

When 0.215 g of sodium metal is added to an excess of hydrochloric acid, 2230 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HC1(aq) 2 NaCI(aq) + H, (g) Enthalpy of reaction: kJ