The heat of combustion for butane, C4H10, is 45.7 kJ/g. How much heat is produced if 4.0 moles of butane undergo complete combustion? Express your answer in kilojoules and enter only the number (no units).
Added by Julia G.
Step 1
01 g/mol Molar mass of H = 1.008 g/mol Molar mass of butane (C4H10) = 4(12.01) + 10(1.008) = 58.12 g/mol Show more…
Show all steps
Your feedback will help us improve your experience
Ronald Prasad and 88 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
How many grams of butane C4H10 must be burned to produce 3.50 X 104 kJ of heat? 2 C4H10 + 13 O2 ⟶⟶ 8 CO2 + 10 H2O ΔΔ H = - 5,755 kJ Molar mass of butane is 58.14 g / mole
Shaiju T.
Combustion reactions are exothermic. The heat of reaction for the combustion of butane (C4H10) is 687.8 kcal/mol. What is the heat of combustion for butane in kcal/gram? How much heat will be given off if molar quantities of butane react according to the following equation: 2 C4H10 + 13 O2 -> 8 CO2 + 10 H2O?
Dominique Jan T.
When $1.000 \mathrm{~g}$ of gaseous butane, $\mathrm{C}_{4} \mathrm{H}_{10}$, is burned at $25^{\circ} \mathrm{C}$ and 1.00 atm pressure, $\mathrm{H}_{2} \mathrm{O}(l)$ and $\mathrm{CO}_{2}(g)$ are formed with the evolution of $49.50 \mathrm{~kJ}$ of heat. a.Calculate the molar enthalpy of formation of butane. (Use enthalpy of formation data for $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{CO}_{2} .$ ) b.$\Delta G_{f}^{\circ}$ of butane is $-17.2 \mathrm{~kJ} / \mathrm{mol}$. What is $\Delta G^{\circ}$ for the combustion of $1 \mathrm{~mol}$ butane? c.From a and b, calculate $\Delta S^{\circ}$ for the combustion of 1 mol butane.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD