Given the data:  N2H4(l) + O2 (g) → N2(g) + 2 H2O (l) ΔH° = – 622.2 kJ 2 H2(g) + O2 (g) → 2H2O (l) ΔH° = -571.6 kJ H2(g) + O2 (g) → H2O2(l) ΔH° = – 187.8 kJ   using Hess’s Law the ∆H for the reaction below is [a] kJ:N2H4 (l) + 2 H2O2 (l) → N2(g) + 4 H2O (l)Must show your work (scratch paper) to receive credit.

When a 2.150-g sample of glucose, C6H12O6, is burned in a bomb calorimeter with a heat capacity of 6.317 kJ/°C, the temperature of the calorimeter increases from 23.446°C to 28.745°C. Calculate ∆E for the combustion of glucose in kJ/mol.

Given the following equations and ∆H° values:                                                               OF2(g) + H2O(l) → O2(g) + 2 HF(g) ∆H° = -276.6 kJ SF4(g) + 2 H2O(l) → 4 HF(g) + SO2(g) ∆H° = -827.5 kJ S(s) + O2(g) → SO2(g) ∆H° = -296.9 kJ  determine the heat of reaction (kJ) at 298 K for the reaction:  2 OF2(g) + 2 S(s) →SO2(g) + SF4(g) Must show your work (scratch paper) to receive credit.

Use the standard enthalpies of formation provided to calculate the change in enthalpy for the reaction below: 5 CO(g)  +  11 H2(g) → C5H12(l)   + 5 H2O(l)      ΔH°f (kJ/mol) CO(g)  – 110.5 H2O(l)  – 285.8 C5H12(l)    – 146.8 Must show your work (scratch paper) to receive credit.

Use the standard enthalpies of formation provided to calculate the change in enthalpy for the reaction below: 5 CO(g)  +  11 H2(g) → C5H12(l)   + 5 H2O(l)      ΔH°f (kJ/mol) CO(g)  – 110.5 H2O(l)  – 285.8 C5H12(l)    – 146.8 Must show your work (scratch paper) to receive credit.

Write the condensed (short form) electron configuration for Hf:( Make sure to follow the order following the Aufbau principle. Do not consider exceptions. Do not use superscripts, do not write the brackets on the noble gas. Use the following format Ne – 3s2 ….)

Sodium metal can react vigorously with water. How much heat evolved with 15.0 g of metallic sodium are thrown in a bucket of water as determined by the following reaction: Must show your work (scratch paper) to receive credit. 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) +  H2(g)     ΔH°rxn = – 368.4 kJ

A reactive element with a relatively high electronegativity would be expected to have a relatively

Use Hess’s Law and the following data   CH4(g) + 2 O2(g) → CO2(g)   +  2 H2O(g) ΔH = −802 kJ CH4(g) + CO2(g) → 2 CO(g)   +  2 H2(g) ΔH = + 247 kJ CH4(g) + H2O(g) → CO(g)   +  3 H2(g) ΔH = + 206 kJ   to determine the ∆H°rxn for the following reaction, an important source of hydrogen gas:   2 CH4(g) + O2(g) →  2 CO(g)   +  4 H2(g)   Must show your work (scratch paper) to receive credit.

Which depends only on the initial and final state?