How much heat will be released when 12.0 g of #H_2# reacts with 76.0 g of #O_2# according to the following equation? #2H_2 + O_2 - 2H_2O# #DeltaH#= -571.6 kJ?

Question

How much heat will be released when 12.0 g of #H_2# reacts with 76.0 g of #O_2# according to the following equation?  #2H_2 + O_2 -> 2H_2O#  #DeltaH#= -571.6 kJ?

Olivia Anton · Accepted Answer

#"Dioxygen gas"# is the limiting reagent. Over #1.3xx10^3*kJ# are evolved.

#2H_2(g) + O_2(g) rarr 2H_2O(l)# #DeltaH=-576.6*kJ*mol^-1.# #"Moles of dihydrogen"=(12.0*g)/(2.016*g*mol^-1)=5.95*mol#. #"Moles of dioxygen"=(76.0*g)/(32.0*g*mol^-1)=2.38*mol#. Given the stoichiometry, clearly, there is a insufficient molar quantity of dioxygen for complete combustion. At most #4.75*mol# dihydrogen can react (i.e. #2xx2.38*mol)# according to the given equation. And thus energy released can based on the molar quantity of #"dioxygen gas"# #=# #2.38*molxx-576.6*kJ*mol^-1=??kJ#

Jose Ayala · Answer

undefined First, calculate the moles of H₂ and O₂. Then, determine the limiting reactant. Finally, use the stoichiometry of the reaction and the given enthalpy change to find the heat released. The balanced equation tells us that 2 moles of H₂ react with 1 mole of O₂ to produce 2 moles of H₂O. Calculate the moles of H₂ and O₂:

Moles of H₂ = mass of H₂ (in grams) / molar mass of H₂
Moles of O₂ = mass of O₂ (in grams) / molar mass of O₂

Then, determine the limiting reactant. Compare the moles of each reactant to the stoichiometric ratio in the balanced equation. The limiting reactant will be the one that is completely consumed.

Once you have identified the limiting reactant, use the stoichiometry of the reaction to find the moles of water produced. Then, use the given enthalpy change to calculate the heat released. The enthalpy change is given per mole of reaction, so multiply the moles of reaction by the enthalpy change to find the total heat released.

Peyton Adams · Answer

undefined To find the amount of heat released, you need to calculate the moles of hydrogen and oxygen reacting, then use the stoichiometry of the reaction to determine the amount of heat released.

1. Calculate the moles of hydrogen ($H_2$) and oxygen ($O_2$):
   Moles of $H_2$ = mass of $H_2$ / molar mass of $H_2$
   Moles of $O_2$ = mass of $O_2$ / molar mass of $O_2$

2. Determine the limiting reactant (the reactant that will be completely consumed).

3. Use the stoichiometry of the reaction to find the moles of water ($H_2O$) produced from the limiting reactant.

4. Apply the molar enthalpy of reaction to find the amount of heat released:
   Heat released = moles of water produced × molar enthalpy of reaction.

Here are the calculations:

1. Moles of $H_2$:
   Moles of $H_2$ = 12.0 g / 2.016 g/mol

2. Moles of $O_2$:
   Moles of $O_2$ = 76.0 g / 31.998 g/mol

3. Determine the limiting reactant:
   From the stoichiometry of the reaction, 2 moles of $H_2$ react with 1 mole of $O_2$. Calculate the moles of water that can be formed from each reactant and identify the limiting reactant.

4. Calculate the moles of water produced:
   Moles of $H_2O$ = (moles of limiting reactant) × 2 (since 2 moles of $H_2O$ are produced for every 2 moles of $H_2$ consumed)

5. Calculate the heat released:
   Heat released = (moles of water produced) × (-571.6 kJ/mol)

Performing the calculations will give you the amount of heat released.

HIX Tutor · Answer

undefined To calculate the amount of heat released when a reaction occurs, you need to use the equation Q = m × ΔH, where Q represents heat, m represents the mass of the substance reacting, and ΔH represents the heat of the reaction.

Step 1: Determine the limiting reactant
To find the limiting reactant, compare the number of moles of each reactant to the stoichiometric ratio in the balanced equation. The reactant that produces fewer moles of the product is the limiting reactant.

Step 2: Calculate the moles of the limiting reactant
Convert the mass of the limiting reactant to moles using the molar mass. The molar mass of H₂ is 2 g/mol, and the molar mass of O₂ is 32 g/mol.

Step 3: Determine the heat released
Multiply the moles of the limiting reactant by the ΔH value from the balanced equation.

Step 4: Convert heat to kilojoules
Since the ΔH value is given in kilojoules, there is no need for additional conversion.

Step 5: Round your answer
Round the final answer to the correct number of significant figures based on the given values.

I hope this answer helps! Is there anything else you would like to know?

How much heat will be released when 12.0 g of #H_2# reacts with 76.0 g of #O_2# according to the following equation? #2H_2 + O_2 -&gt; 2H_2O# #DeltaH#= -571.6 kJ?

How much heat will be released when 12.0 g of #H_2# reacts with 76.0 g of #O_2# according to the following equation? #2H_2 + O_2 -> 2H_2O# #DeltaH#= -571.6 kJ?