Question

If hydrogen were used as a fuel, it could be burned according to the following reaction:...

If hydrogen were used as a fuel, it could be burned according to the following reaction:
H2(g)+1/2O2(g)→H2O(g)

Use average bond energies to calculate ΔHrxn for this reaction.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

The deltaHrxn = -243 kJ/mol the deltaHrxn of CH4(methane) = -802 kJ/mol

The fuel that yields more energy per mole is METHANE. The negative sign merely signifies the release of energy. Thus, 802 kJ/mol is greater than 243 kJ/mol.

The fuel that yields more energy per gram is HYDROGEN. Here is the computation:

deltaHrxn = (-243 kJ/mol)(1 mol/2.016 g H2) = -120.535714286 kJ/g or -121 kJ/g

deltaHrxn of CH4(methane) = (-802 kJ/mol)(1 mol/16.04 g)

= -50 kJ/g

As discussed the negative sign serves as the symbol of released energy. Thus, 121 is greater than 50.

Read more on Brainly.com - https://brainly.com/question/1577933#readmore

0 0
Know the answer?
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

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Gaseous hydrogen can be used as a clean fuel since it only produces water according to...
Gaseous hydrogen can be used as a clean fuel since it only produces water according to the following fuel reaction: H2 (g) + O2 (g) = H2O (g) If this reaction has a 98% experimental yield, determine the necessary mass of H2 to produce 1000.0 kg of water.
Hydrogen gas can be used as a clean fuel since it only produces water according to...
Hydrogen gas can be used as a clean fuel since it only produces water according to the next fuel reaction: H2 + O2 = H2O if this reaction has a 98% experimental yield, determine the mass of H2 to produce 1000.0 kg of water.
The major industrial source of hydrogen gas is by the following reaction: CH4(g) + H2O(g) ------>...
The major industrial source of hydrogen gas is by the following reaction: CH4(g) + H2O(g) ------> CO(g) + 3 H2(g) Use bond energies to predict deltaH for this reaction. So I used bond energy chart: CH4(g): 4mol C-H= 4*413kJ/mol H2O(g): 2mol H-O = 2*467kJ/mol 3 H2(g): 3mol H-H = 3*432kJ/mol CO(g): 1mol C-O = 1*358kJ/mol And I got the answer as 1290kJ.... but it is wrong because apparently for CO(g) the bond has to be a triple bond...so the energy...
Hydrogen is oxidized in a fuel cell to make electricity, by the (unbalanced) reaction: H2 +...
Hydrogen is oxidized in a fuel cell to make electricity, by the (unbalanced) reaction: H2 + O2  H2O. 1 kg/min H2 is fed to the fuel cell, and oxygen is fed as 21% of air. The oxygen is fed at a rate 50% more than the minimum required to completely oxidize all the H2. Assuming that all the Hydrogen is consumed, find the molar flow rate of all chemical species leaving the fuel cell.
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)→CO(g)+3H2(g) In a particular reaction, 26.5 L of methane gas (measured at a pressure of 736 torr and a temperature of 25 ∘C) is mixed with 22.6 L of water vapor (measured at a pressure of 700 torr and a temperature of 125 ∘C). The reaction produces 26.0 L of hydrogen gas measured at STP. What is the percent...
Use the following reaction enthalpies to determine the reaction enthalpy for 2 HCl(g) + F2(g) →...
Use the following reaction enthalpies to determine the reaction enthalpy for 2 HCl(g) + F2(g) → 2 HF(g) + Cl2(g). 4 HCl(g) + O2(g) → 2 H2O(l) + 2 Cl2(g) ΔHrxn = - 202.4 kJ/mol rxn 1/2 H2(g) + 1/2 F2(g) → HF(g) ΔHrxn = - 271.0 kJ/mol rxn H2(g) + 1/2 O2(g) → H2O(l) ΔHrxn = - 285.8 kJ/mol rxn
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water...
Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the following equation: CH4(g)+H2O(g)→CO(g)+3H2(g) In a particular reaction, 26.5 L of methane gas (measured at a pressure of 730 torr and a temperature of 25 ∘C) is mixed with 22.6 L of water vapor (measured at a pressure of 704 torr and a temperature of 125 ∘C). The reaction produces 26.2 L of hydrogen gas measured at STP. What is the percent...
Consider a hydrogen-oxygen fuel cell, an electrochemical cell that generates electricity from the chemical reaction 2...
Consider a hydrogen-oxygen fuel cell, an electrochemical cell that generates electricity from the chemical reaction 2 H2(g) + O2(g) → 2 H2O(l) . Yes, this is the same reaction as in additional question 1, but now we are looking at electrochemical aspects of it. On one side of the cell, H2 is pumped in, and the half-cell reaction is 2 H2(g) + 4 OH–(aq) → 4 H2O(l) + 4 e– ; at the other side, O2 is pumped in: O2(g)...
Diborane (B2H6) reacts with water to form boric acid (H3BO3) and hydrogen gas (H2) according to...
Diborane (B2H6) reacts with water to form boric acid (H3BO3) and hydrogen gas (H2) according to the following reaction: B2H6(g) + 6H20(L)----> 2H3BO3(s)+ 6H2(g) [Molar Masses (g/mol): B2H6:27.67, H2O: 18.02, H3BO3: 61.83, H2:2.02] a.) In a particular experiment 18.0 mol of H2O are consumed, how many mol of H3BO3 were produced? b.) Calculate the mass (in g) of B2H6 needed to produce 278.2g of H3BO3 (assuming excess H2O)
Ethanol is a possible fuel. Use average bond energies to calculate ?Hrxn for the combustion of...
Ethanol is a possible fuel. Use average bond energies to calculate ?Hrxn for the combustion of ethanol. CH3CH2OH(g) + 3 O2(g) ? 2 CO2(g) + 3 H2O(g)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT