How do you balance the equation for the reaction with an energy term in kcal as...

Question

Question

How do you balance the equation for the reaction with an energy term in kcal as part of the equation?

When N2(g) reacts with O2(g) to form NO2(g), 15.9 kcal of energy is absorbed for each mole of N2(g) that reacts.

When Fe2O3(s) reacts with Al(s) to form Al2O3(s) and Fe(s), 204 kcal of energy is evolved for each mole of Fe2O3(s) that reacts.

When CO2(g) reacts with H2(g) to form CO(g) and H2O(g), 9.85 kcal of energy is absorbed for each mole of CO2(g) that reacts.

science chemistry

Answer 1

Answer #1

When energy is absorbed it will added with left hand side reactant.

When energy is released or evolved it will be added with right hand side product.

a) N46+202 (9) —> 2N02 9) As heat is absorbed, it will on L.H.S. energy N₂ (9) + 20 (9) + 15.9 kcal 2 NO₂(g) | N2(g) +202 (9)

c) CO2 (9)+H2(g) +9.85 kcal → C009) 7. H2009)

Answer 2

Similar Homework Help Questions

When H2S(g) reacts with H2O(l) to form H2(g) and SO2(g) , 70.5 kcal of energy are...

When H2S(g) reacts with H2O(l) to form H2(g) and SO2(g) , 70.5 kcal of energy are absorbed for each mole of H2S(g) that reacts. Write a balanced equation for the reaction with an energy term in kcal as part of the equation.
When H2(g) reacts with C2H4(g) to form C2H6(g), 32.7 kcal of energy are evolved for each...

When H2(g) reacts with C2H4(g) to form C2H6(g), 32.7 kcal of energy are evolved for each mole of H2(g) that reacts. Write a balanced equation for the reaction with an energy term in kcal as part of the equation.
When Fe_2O_3(s) reacts with Al(s) to form Al_2O_3(s) and Fer(s).204 kcal of energy are evolved for...

When Fe_2O_3(s) reacts with Al(s) to form Al_2O_3(s) and Fer(s).204 kcal of energy are evolved for each mole of Fe_2O_39s) that reaction Write a balanced equation the reaction with an energy term in local as part of the equation. Use the SMALLEST INTEGER coefficients possible and put the energy term in an appropriate box. If a box is not accord, leave it blank.

. Use the equation below to calculate how much heat (in kJ) is evolved when 5.0...

. Use the equation below to calculate how much heat (in kJ) is evolved when 5.0 g of aluminium reacts with a stoichiometric amount of Fe2O3? 2 Al (s) + Fe2O3 (s) —>2 Fe (s) + Al2O3 (s) AH° = -852 kJ Determine the AHPrxn for the following reaction. {AH® (NH3) = -45.9 kJ/mol; AH°(O2) = 0; AH® (NO) = +91.3 kJ/mol; AH° (H2O) = -241.8 kJ/mol; 4 NH3 (g) + 5 O2 (g) — 4 NO (g) + 6...
5.) How much energy is evolved during the reaction of 4.00 moles of Al, according to...

5.) How much energy is evolved during the reaction of 4.00 moles of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) Hºrxn = -852 kJ/mole (remember, AH°rxn is referenced to the whole chemical equation as one mole unit)
5.) How much energy is evolved during the reaction of 4.00 moles of Al, according to...

5.) How much energy is evolved during the reaction of 4.00 moles of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) Hºrxn = -852 kJ/mole (remember, AH°rxn is referenced to the whole chemical equation as one mole unit)

Please help with these two questions :( 1. How much energy (in kJ) is evolved during...

Please help with these two questions :( 1. How much energy (in kJ) is evolved during the reaction of 76.9 g of Al, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ Assume that there is excess Fe2O3. 2. A 12.43 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter with a heat capacity, C = 5.65 kJ/°C. C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn...
In each case, find the missing ∆Hºrxn(kJ/mole) &n

In each case, find the missing ∆Hºrxn(kJ/mole) a. If 2 Al(s) + Fe2O3(s) ---- > Al2O3(s) + 2 Fe(s) ΔHrxno = -851.5kJ/mol then 1/8 Al2O3(s) + 1/4 Fe(s) --- > 1/4 Al(s) + 1/8 Fe2O3(s) ΔHrxno = ? b. If CaO(s) + 3 C(s) --- > CaC2(s) + CO(g) ΔHrxno = 464.8 kJ/mol then 6 CaO(s) + 18 C(s) --- > 6 CaC2(s) + 6 CO(g) ΔHrxno = ? ...
How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below

How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s), ΔH°rxn = -852 kJ

3.(15pts) In each case, find the missing AH. (kJ/mole) (a) If 2 Al(s) + Fe2O3(s) ---->...

3.(15pts) In each case, find the missing AH. (kJ/mole) (a) If 2 Al(s) + Fe2O3(s) ----> Al2O3(s) + 2 Fe(s) AH,xº = -851.5kJ/mol then 1/8 Al2O3(s) + 1/4 Fe(s) --> 1/4 Al(s) + 1/8 Fe2O3(s) AHX = ? (b) If CaO(8) + 3 C(s) --> CaC2(s) + CO(g) AH,” = 464,8 kJ/mol then 6 CaO(s) + 18 C(s) ---> 6 CaCz(s) +6 CO(g) AHX = ? (c) If N2(g) + 2 O2(g) ---> N204(g) and 2 NO2(g) ----> N2(g) +...