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.

Write the full electron configuration for Ti: (Do not consider exceptions. Make sure to follow the order following the Aufbau principle, use the following format without superscripts: 1s2 2s2 2p6…)

A coffee-cup calorimeter contains 100.0 mL of 1.000 M HCl (excess) at 20.3 °C. When 1.82 g Zn(s) is added, the temperature rises to 30.5 °C. What is the heat of reaction per mol Zn? Assume that the heat of solution is that of water, and the density of the HCl is 1.000 g/mL.   Zn(s)  + 2 HCl(aq)  → ZnCl2(aq)  + H2(g)   

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