Please Solve all question with all the work How much heat is liberated when 0.11

Question

Please Solve all question with all the work

How much heat is liberated when 0.113 moles of sodium reacts with excess water according to the following equation? 2 Na_(s) + 2 H_2 O_(l) rightarrow H_2 (g) + 2 Na OH _(aq) delta H = -368 kJ/mol rxn 2. How much heat energy is required to convert 74.6g of lead(II) oxide to lead according to the following equation? PbO_(s) + C(s) rightarrow Pb_(s) + CO_(g) delta H = +107kJ/mol rxn Using the following thermochemical equation, CH_3 OH_(g) + 3/2 O_2 (g) rightarrow CO_2 (g) + H_2 O_(l) delta H = -764 kJ/mol rxn (a) How much heat is evolved when 90.0g of CH_3 OH bums in excess oxygen. (b) What mass of O_2 is consumed when 945kJ of heat energy is released?

Explanation / Answer

1. Given the equation: 2Na + 2H2O ===> H2 + 2NaOH

2 moles of Na produces heat = -368kJ as given dH for this reaction is -368kJ/mol reaction.

So, 1mol Na will produce heat = -368/2 = -184kJ/mol

So, 0.113moles of Na will produce heat = 0.113 x 184 = -20.79 kJ/mol

Heat for 0.113moles Na = -20.79kJ

Have a nice day!! :)

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