Solve this Standard Heat of Reaction Problem

Given the standard heats of formation for the following compounds, calculate the change H2 degrees 98 for the following reaction CH4 (g) + H2O (g) >>>>>> CH3OH (l) + H2 (g) Change in H Degree F (kj/mole) -75 -242 -238 0 I need to see how to solve this, and most importantly, the answer

Heat (in Kj/mol rxn) absorption in this reaction

How much heat is absorbed in the complete reaction of 3.00 grams of SiO2 with excess carbon in the reaction below? Change in H degrees for the reaction is +624.6 kJ. SiO2 (g) + 3C (s) >>>>>>> SiC (s) + 2CO (g)

Delta Heat for a reaction

Evaluate Delta H (standard) for the reaction below at 25 degress celcius SiO2 (s) + 4HF (aq) >>>>>>> SiF4 (g) + 2H2O (l) DeltaH standard f (kj/mol) -910.9 -320.8 -1615 -285.8

Specific Rate Constant

Evaluate the specific rate constant for the reaction at the temperature for which the data were obtained. The rate-law expression is rate=k[A][B]squared. A + B>>>>>> C Experiment Initial [A] Initial [B] Initial Rate of Formation of C 1 0.10 M 0.10 M 4.0 X .00010 M/min 2 0.20 M 0.20 M 3.2 X .0010 M/min 3 0.10 M 0.20 M 1.6 X .0010 M/min

Half-Life

At 300 K the reaction below obeys the rate law Rate=k[NOCl]squared where k=2.8 X .000010 M to the neg 1 times s to the neg 1. 2 NOCl >>>>>> 2NO + Cl2 Suppose 1.0 mole of NOCl is introduced into a 2.0-liter container at 300 K. Evaluate the half-life of the reaction.