A scientist measures the standard enthalpy change for the following reaction to be -351.2 kJ : P,O10(s) + 6 H,O(1)- →4H3PO (aq) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of P,010(s) is kJ/mol.

Using standard heats of formation, calculate the standard enthalpy change for the following reaction. ΔΗ° rxn 4NH3(g) +502 (g) → 4NO(g) + 6H₂O(g) AH (NH3 (9)) = -46.1 kJ/mol AH (O₂ (g)) = 0.0 kJ/mol AH (NO(g)) = 90.3 kJ/mol AH (H₂O(g)) = -241.8 kJ/mol = KJ

2. Cold packs take advantage of the fact that dissolving NH4NO3 in water is an endothermic process. When 5.44 g of solid ammonium nitrate is added to 150.0 g of water in a coffee cup calorimeter, the temperature of the solution changes from 18.6 °C to a final temperature which you will determine. Calculate the enthalpy change for dissolving ammonium nitrate in water, in kJ/mol. Assume the specific heat of the solution is 4.2 J/g·K.g. Using the value of qsolution, calculate ∆T, as well as the final temperature reached by the solution.

The reaction of iron with oxygen is a common occurrence. You can observe the resulting rust on buildings, vehicles and bridges. However, you may find the large amount of heat produced by this reaction surprising. 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)                      ΔHorxn = -1.65 x 103 kJ a) Rewrite the thermochemical equation to include the enthalpy change as a term in the equation. b) What is the enthalpy change associated with the formation of 23.6 g of iron (III) oxide?

A scientist measures the standard enthalpy change for the following reaction to be 215.5 kJ : CH4(g) + H20(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 H,O(g) is kJ/mol.

A chemist measures the enthalpy change AH during the following reaction: 2 Al(s) + Fe,03(s)→ Al,O3(s) + 2 Fe(s) AH=-852. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. ol. reaction ΔΗ Ar 4Al (s) + 2Fe,O,(s) → 2Al,0, (s) + 4Fe(s) Al, 0, (s) + 2Fe(s) 2A1 (s) + Fe, 03 (s) |kJ 3 Al,0, (s) + 6Fe(s) → 6A1(s) + 3Fe,0, (s) kJ Explanation Check © 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

For the reaction H,(2) + 0,) → H,0M AH = - 286KJ/mol Calculate the enthalpy change when 2.50 g of water is produced.

When a 4.456-g sample of margarine is burned with excess oxygen in a bomb calorimeter with a heat capacity of 22.35 kJ·K–1. The temperature of the calorimeter rises from 18.76°C to 37.75°C. What is the ΔUrxn value, in units of kJ/g, for the combustion of this margarine sample?  correct amount of significant figures.

Carbon disulfide is a colorless liquid. When pure, it is nearly odorless, but the commercial product smells vile. Carbon disulfide is used in the manufacture of rayon and cellophane. The liquid burns as follows: CS2(ℓ) + 3O2(g) → CO2(g) + 2SO2(g) Calculate the standard enthalpy change for this reaction using standard enthalpies of formation. ΔH°f (CS2(ℓ)) = 89.70 kJ ΔH°f (CO2(g)) = -393.52 kJ ΔH°f (SO2(g)) = -296.8 kJ

Methanol can be synthesized from graphite according to the following reaction, calculate the enthalpy change, in kJ/mol, for the overall reaction: 2C(graphite) + 4H2(g) + O2(g) → 2CH3OH(l) Using the data given below: C(graphite) + O2(g) → CO2(g)     ΔrH = -393.5 kJ/mol 2H2(g) + O2(g) → 2H2O(l)     ΔrH = -571.6 kJ/mol 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l)     ΔrH = -1452.8 kJ/mol (Enter the numerical value in the space provided below, be sure to include the negative sign if needed.