What mass of butane in grams is necessary to produce 1.5 × 10^3 kJ of heat? What mass of CO2 is produced? C4H10(g) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(g)       ΔH rxn = –2658 kJ

Expert Answers

An illustration of the letter 'A' in a speech bubbles

The change in enthaply of the reaction (delta H) is -2658 kJ.  This means that 2658 kJ of heat is released from the exothermic reaction.  From the chemical equation, we see that this amount is for a single mole of butane since the coefficient in front of the butane (C4H10) is 1.  So for...

(The entire section contains 149 words.)

Unlock This Answer Now

Start your 48-hour free trial to unlock this answer and thousands more. Enjoy eNotes ad-free and cancel anytime.

Start your 48-Hour Free Trial
Approved by eNotes Editorial Team