HomeworkLib
Question

Pentaborane-9, B5H9, is a colorless, highly reactive liquid that will burst into flame when exposed to...

Pentaborane-9, B5H9, is a colorless, highly reactive liquid that will burst into flame when exposed to oxygen. The reaction is:

2 B5H9 (l)+ 12 O2 (g)-----> 5 B2O3 (s)+ 9 H2O (l)

∆Hfº = -8890.2 kJ/mol Calculate the kilojoules of heat released per gram of the compound reacted with oxygen

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Request Professional Answer

Request Answer!

We need at least 10 more requests to produce the answer.

0 / 10 have requested this problem solution

The more requests, the faster the answer.

Request! (Login Required)

All students who have requested the answer will be notified once they are available.
Know the answer?
Add Answer to:
Pentaborane-9, B5H9, is a colorless, highly reactive liquid that will burst into flame when exposed to...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Similar Homework Help Questions

  • Calculate the kJ of heat per gram released by Pentaborane-9?

    Pentaborane-9 (B5H9) is a colorless, highly-reactive liquid that will burst into flames when exposed to oxygen.The reaction is:2B5H9 (l) + 12O2 (g) --> 5B2O3 (s) + 9H2O (l)Calculate the kilojoules of heat released per gram of the compound reacted with oxygen.The standard enthalpy of formations of B5H9 (l), B2O3 (s), and H2O(l) are 42.84, -1271.94, and -285.83 kJ/mol, respectively.

  • (a) Diborane (B2H6) is a highly reactive borohydride that can be used as rocket fuel. Calculate Δ? for synthesis from th...

    (a) Diborane (B2H6) is a highly reactive borohydride that can be used as rocket fuel. Calculate Δ? for synthesis from the elements as: 2B (s) + 3H2 (g) → B2H6 (g) Use the following data: 4B (s) + 3O2 (g) → 2B2O. (S) Δ? = -2546 kJ mol-1 B2H6 (g) + 3O2 (g) → B2O3 (s) + 3H2O (g) Δ? = -2035 kJ mol-1 2H2 (g) + O2 (g) → 2H2O (l) Δ? = -572 kJ mol-1 H2O (l) →...

  • When styrene C8H8 burns in oxygen to form carbon dioxide and liquid water under standard-state conditions...

    When styrene C8H8 burns in oxygen to form carbon dioxide and liquid water under standard-state conditions at 25°C, 42.62 kJ are released per gram of styrene. Find the standard enthalpy of formation of styrene at 25°C. (Given: ΔH°f[CO2(g)] = –393.5 kJ/mol, ΔH°f[H2O(l)] = –285.8 kJ/mol)

  • The gas ethane, C2H6(g), can be used in welding. When ethane is burned in oxygen, the...

    The gas ethane, C2H6(g), can be used in welding. When ethane is burned in oxygen, the reaction is: 2 C2H6(g) + 7 O2(g)4 CO2(g) + 6 H2O(g) (a) Using the following data, calculate ΔH° for this reaction. ΔH°f kJ mol-1: C2H6(g) = -84.0 ; CO2(g) = -393.5 ; H2O(g) = -241.8 ΔH° = kJ (b) Calculate the total heat capacity of 4 mol of CO2(g) and 6 mol of H2O(g), using CCO2(g) = 37.1 J K-1 mol-1 and CH2O(g) =...

  • The compound 1-propanol, C3H8O, is a good fuel. It is a liquid at ordinary temperatures. When...

    The compound 1-propanol, C3H8O, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is 2 C3H8O(ℓ) + 9 O2(g)6 CO2(g) + 8 H2O(g)   The standard enthalpy of formation of liquid 1-propanol at 25 °C is -302.6 kJ mol-1; other relevant enthalpy of formation values in kJ mol-1 are:   C3H8O(g) = -255.1 ; CO2(g) = -393.5 ; H2O(g) = -241.8 (a) Calculate the enthalpy change in the burning of 3.000 mol...

  • The compound heptane, C7H16, is a good fuel. It is a liquid at ordinary temperatures. When...

    The compound heptane, C7H16, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is C7H16(ℓ) + 11 O2(g)7 CO2(g) + 8 H2O(g) The standard enthalpy of formation of liquid heptane at 25 °C is -224.2 kJ mol-1; other relevant enthalpy of formation values in kJ mol-1 are: C7H16(g) = -187.6 ; CO2(g) = -393.5 ; H2O(g) = -241.8 (a) Calculate the enthalpy change in the burning of 2.000 mol liquid...

  • The compound 1-pentanol, C5H12O, is a good fuel. It is a liquid at ordinary temperatures. When...

    The compound 1-pentanol, C5H12O, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is 2 C5H12O(ℓ) + 15 O2(g)10 CO2(g) + 12 H2O(g) The standard enthalpy of formation of liquid 1-pentanol at 25 °C is -351.6 kJ mol-1; other relevant enthalpy of formation values in kJ mol-1 are: C5H12O(g) = -294.6 ; CO2(g) = -393.5 ; H2O(g) = -241.8 (a) Calculate the enthalpy change in the burning of 5.000 mol...

  • Use the set of three reactions shown below to answer the questions that follow. 2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ 2N...

    Use the set of three reactions shown below to answer the questions that follow. 2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ 2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJ N2(g) + O2(g) → 2NO(g) ΔH = +183 kJ a. If 30.2 g of NO g is reacted with excess oxygen, how much heat energy is produced? b. What mass of liquid water will be consumed during the production of 31000 J of energy assuming that...

  • can you do the 7 and 9 ? can you also show and explain me step...

    can you do the 7 and 9 ? can you also show and explain me step by step? D. 49.6 kJ E. 57.3 kJ 7. Butane (C4H10) undergoes combustion in excess oxygen to generate gaseous carbon dioxide and water. Given AH° [C4H10(g)] = -124.7 kJ/mol, AH° [CO2(g)] = -393.5 kJ/mol, AH [H2O(g)] = -241.8 kJ/mol, how much energy is released (kJ) when 8.30 g of butane is burned? Combustion of butane: 2 CH2(g) + 13 O2(g) → 8 CO2(g) +...

  • Use the set of three reactions shown below to answer the questions that follow. 2NO(g) +...

    Use the set of three reactions shown below to answer the questions that follow. 2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ 2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJ N2(g) + O2(g) → 2NO(g) ΔH = +183 kJ If 27.9 g of NO g is reacted with excess oxygen, how much heat energy is produced? What mass of liquid water will be consumed during the production of 33900 J of energy assuming that there is...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT