Which statement about this reaction is correct?

13.3 KJ of energy are absorbed for every mole of Fe reacted

26.6 KJ of energy are released for every mole of Fe reacted

26.6 KJ of energy are absorbed for every mole of Fe reacted

53.2 KJ of energy are released for every mole of Fe reacted

When solutions of HCl and NaOH are mixed the temperature increases. The reaction:

is exothermic with a negative enthalpy energy

is endothermic with a positive enthalpy energy

is endothermic with a negative enthalpy energy

is exothermic with a positive enthalpy energy

What can be deduced about the relative stability of the reactants and products and the sign of from the enthalpy level diagram above?

Reactants are more stable and sign of difference of enthalpy energy is positive

Products are more stable and sign of difference of enthalpy energy is negative

Products are more stable and sign of difference of enthalpy energy is positive

Reactants are more stable and sign of difference of enthalpy energy is negative

The enthalpy difference for the third reaction must be negative and larger than 52.3 KJ

The enthalpy difference for the third reaction must be negative

The enthalpy difference for the third reaction must be positive and smaller than 52.3 KJ

No conclusion can be made without the value of H and H2(g)

What energy changes occur when chemical bonds are formed and broken?

energy is released when bonds are formed and absorbed when they are broken

energy is absorbed when bonds are formed and when they are broken

energy is released when bonds are formed and when they are broken

energy is absorbed when bonds are formed and released when they are broken

Which statement about this reaction is correct? 2Fe(s) + 3CO2 (g) -> Fe2O3(s) + 3CO(g) DH = +26.6 kJ

13.3 kJ of energy are absorbed for every mole of Fe reacted

26.6 kJ of energy are released for every mole of Fe reacted

26.6 kJ of energy are absorbed for every mole of Fe reacted

53.2 kJ of energy are released for every mole of Fe reacted

Which statement about exothermic reactions is not correct?

The products have a greater enthalpy than the reactants

The enthalpy change (∆H) is negative

The products are more stable than the reactants

When solid ammonium nitrate dissolves in water, the temperature decreases. Which statement about the dissolving of ammonium nitrate in water is correct?

It is endothermic with ∆H greater than zero.

It is endothermic with ∆H less than zero.

It is exothermic with ∆H less than zero.

It is exothermic with ∆H greater than zero.

Which statement about endothermic reactions is not correct?

They have positive ∆H values.

Products have a higher enthalpy than the reactants.

Products are less thermally stable than the reactants.

IBSL Chemistry Topic 5 Energetics Multiple Choice Questions

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IBSL Chemistry Topic 5 Energetics Multiple Choice Questions

Which statement about this reaction is correct?

When solutions of HCl and NaOH are mixed the temperature increases. The reaction:

What can be deduced about the relative stability of the reactants and products and the sign of from the enthalpy level diagram above?

For the reaction: IF

The enthalpy changes for two different hydrogenation reactions of Which expression represents the enthalpy change for the reaction below?

Use the bond energies for H-H (346kJ.mol-1) Br-Br (193 Kj mol-1) and H-Br (366 KJ mol-1) to calculate (in KJ mol-1) for the reaction:

The average bond enthalpy for the C-H bond is 412 KJ mol-1. Which process has an enthalpy change closest to this value?

What energy changes occur when chemical bonds are formed and broken?

The temperature of a 2.0g sample of aluminium increases from 25 to 30 degrees Celsius. How many joules of heat energy were added? Specific Heat Capacity of Al= 0.90 J.g-1. K-1

Using the eqautions below:

Question No Image

The average bond enthalpies for O-O and for O=O are 146 and 496 KJ.mol-1 repectively. What is the enthalpy change, in KJ, for the reaction below? H-O-O-H (g) --> H-O-H (g) + 1/2 O=O (g)

The enthalpy changes for two different hydrogenation reactions of C₂H₂ are; C₂H₂ + H₂ ->C₂H₄ DH₁ C₂H₂ +2H₂ -> C₂H₆ DH₂ Which expression represents the enthalpy change for the reaction below? C₂H₄ + H₂ -> C₂H₆ DH=?

The bond enthalpies of H₂, Br₂ and HBr are 436, 192, and 366 kJ mol^-1 respectively. Use these values to calculate ∆H in kJ for the reaction; H₂ (g) + Br₂ (g) -> 2HBr(g)

N₂ (g) + O₂ (g) à 2NO(g) DH =180.4 kJ N₂ (g) + 20₂ (g) -> 2NO₂ (g) DH = 66.4 kJ Use the enthalpy values above to calculate DH for the reaction: NO(g) + ½ O₂ (g) -> NO₂ (g)

Which statement about this reaction is correct? 2Fe(s) + 3CO₂ (g) -> Fe₂O₃(s) + 3CO(g) DH = +26.6 kJ

Which statement about exothermic reactions is not correct?

Some average bond enthalpies (in kJ mol−1) are as follows: H–H =436 , Cl–Cl =242 , H–Cl =431 What is the enthalpy change (in kJ) for the decomposition of hydrogen chloride? 2HCl →H₂ +Cl₂

When solid ammonium nitrate dissolves in water, the temperature decreases. Which statement about the dissolving of ammonium nitrate in water is correct?

When 0.01 mol of solid NaOH is added to 100 cm³ of 1.0 mol dm⁻³ HCl, the temperature increases by ∆T₁. What will be the temperature change, ∆T₂, for a second experiment in which the amount of NaOH and the volume of 1.0 mol dm⁻³ HCl are each doubled?

O₂(g) →2O(g) ∆H= 498 kJ 3O₂ (g) →2O ₃(g) ∆H= 284 kJ Using the information above, what is ∆H for the following equation in kJ?

Which statement about endothermic reactions is not correct?

The enthalpy changes for two reactions involving hydrogen are as follows: C(s) +2H₂ (g) →CH₄(g) ∆H = − 75 kJ H₂(g) →2H(g) ∆H = + 436 kJ What is the enthalpy change (in kJ) for the reaction CH₄ (g) →C(s) +4H(g) A. −947 B. +361 C. +511 D. +947

Which reaction has an enthalpy change equal to four times the bond enthalpy of the C−H bond?

Consider the following reaction: N₂(g) +3H₂ (g) →2NH₃ (g) ∆H^θ=? Bond enthalpies (in kJ mol −1) involved in the reaction are N≡N x H–H y N–H z Which calculation will give the value of ∆H^θ?

Consider the following reactions: CH₃COOH +OH⁻→CH₃COO ⁻+H₂O ∆H^θ =q₁ kJ H⁺ +OH ⁻→H₂O ∆H^θ =q₂ kJ What is the enthalpy change for the reaction CH₃COOH →CH₃COO⁻ + H⁺

If 3600 J of heat is added to 180 g of C₂H₅OH(l), its temperature increases from 18.5^OC to 28.5^OC. What is the specific heat capacity of C₂H₅OH(l) in J/g/^OC ?

Using the information below: H₂(g) + O₂ (g) → H₂O₂ (l) ∆H = − 187.6 kJ 2H₂ (g) + O₂ (g) → 2H₂O(l) ∆H = − 571.6 kJ what is the value of ∆H (in kJ) for 2H₂O₂(l) → 2H₂O(l) + O₂(g)

IBSL Chemistry Topic 5 Energetics Multiple Choice Questions

Which statement about this reaction is correct?

When solutions of HCl and NaOH are mixed the temperature increases. The reaction:

What can be deduced about the relative stability of the reactants and products and the sign of from the enthalpy level diagram above?

For the reaction: IF

The enthalpy changes for two different hydrogenation reactions of Which expression represents the enthalpy change for the reaction below?

Use the bond energies for H-H (346kJ.mol-1) Br-Br (193 Kj mol-1) and H-Br (366 KJ mol-1) to calculate (in KJ mol-1) for the reaction:

The average bond enthalpy for the C-H bond is 412 KJ mol-1. Which process has an enthalpy change closest to this value?

What energy changes occur when chemical bonds are formed and broken?

The temperature of a 2.0g sample of aluminium increases from 25 to 30 degrees Celsius. How many joules of heat energy were added? Specific Heat Capacity of Al= 0.90 J.g-1. K-1

Using the eqautions below:

Question No Image

The average bond enthalpies for O-O and for O=O are 146 and 496 KJ.mol-1 repectively. What is the enthalpy change, in KJ, for the reaction below? H-O-O-H (g) --> H-O-H (g) + 1/2 O=O (g)

The enthalpy changes for two different hydrogenation reactions of C2H2 are; C2H2 + H2 ->C2H4 DH1 C2H2 +2H2 -> C2H6 DH2 Which expression represents the enthalpy change for the reaction below? C2H4 + H2 -> C2H6 DH=?

The bond enthalpies of H2, Br2 and HBr are 436, 192, and 366 kJ mol-1 respectively. Use these values to calculate ∆H in kJ for the reaction; H2 (g) + Br2 (g) -> 2HBr(g)

N2 (g) + O2 (g) à 2NO(g) DH =180.4 kJ N2 (g) + 202 (g) -> 2NO2 (g) DH = 66.4 kJ Use the enthalpy values above to calculate DH for the reaction: NO(g) + ½ O2 (g) -> NO2 (g)

Which statement about this reaction is correct? 2Fe(s) + 3CO2 (g) -> Fe2O3(s) + 3CO(g) DH = +26.6 kJ

Which statement about exothermic reactions is not correct?

Some average bond enthalpies (in kJ mol−1) are as follows: H–H =436 , Cl–Cl =242 , H–Cl =431 What is the enthalpy change (in kJ) for the decomposition of hydrogen chloride? 2HCl →H2 +Cl2

When solid ammonium nitrate dissolves in water, the temperature decreases. Which statement about the dissolving of ammonium nitrate in water is correct?

When 0.01 mol of solid NaOH is added to 100 cm3 of 1.0 mol dm−3 HCl, the temperature increases by ∆T1. What will be the temperature change, ∆T2, for a second experiment in which the amount of NaOH and the volume of 1.0 mol dm−3 HCl are each doubled?

O2(g) →2O(g) ∆H= 498 kJ 3O2 (g) →2O 3 (g) ∆H= 284 kJ Using the information above, what is ∆H for the following equation in kJ?

Which statement about endothermic reactions is not correct?

The enthalpy changes for two reactions involving hydrogen are as follows: C(s) +2H2 (g) →CH4(g) ∆H = − 75 kJ H2(g) →2H(g) ∆H = + 436 kJ What is the enthalpy change (in kJ) for the reaction CH4 (g) →C(s) +4H(g) A. −947 B. +361 C. +511 D. +947

Which reaction has an enthalpy change equal to four times the bond enthalpy of the C−H bond?

Consider the following reaction: N2(g) +3H2 (g) →2NH3 (g) ∆Hθ=? Bond enthalpies (in kJ mol −1) involved in the reaction are N≡N x H–H y N–H z Which calculation will give the value of ∆Hθ ?

Consider the following reactions: CH3COOH +OH−→CH3COO −+H2O ∆Hθ =q1 kJ H+ +OH −→H2O ∆Hθ =q2 kJ What is the enthalpy change for the reaction CH3COOH →CH3COO− + H+

If 3600 J of heat is added to 180 g of C2H5OH(l), its temperature increases from 18.5OC to 28.5OC. What is the specific heat capacity of C2H5OH(l) in J/g/ OC ?

Using the information below: H2(g) + O2 (g) → H2O2 (l) ∆H = − 187.6 kJ 2H2 (g) + O2 (g) → 2H2O(l) ∆H = − 571.6 kJ what is the value of ∆H (in kJ) for 2H2O2(l) → 2H2O(l) + O2(g)

The enthalpy changes for two different hydrogenation reactions of C₂H₂ are; C₂H₂ + H₂ ->C₂H₄ DH₁ C₂H₂ +2H₂ -> C₂H₆ DH₂ Which expression represents the enthalpy change for the reaction below? C₂H₄ + H₂ -> C₂H₆ DH=?

The bond enthalpies of H₂, Br₂ and HBr are 436, 192, and 366 kJ mol^-1 respectively. Use these values to calculate ∆H in kJ for the reaction; H₂ (g) + Br₂ (g) -> 2HBr(g)

N₂ (g) + O₂ (g) à 2NO(g) DH =180.4 kJ N₂ (g) + 20₂ (g) -> 2NO₂ (g) DH = 66.4 kJ Use the enthalpy values above to calculate DH for the reaction: NO(g) + ½ O₂ (g) -> NO₂ (g)

Which statement about this reaction is correct? 2Fe(s) + 3CO₂ (g) -> Fe₂O₃(s) + 3CO(g) DH = +26.6 kJ

Some average bond enthalpies (in kJ mol−1) are as follows: H–H =436 , Cl–Cl =242 , H–Cl =431 What is the enthalpy change (in kJ) for the decomposition of hydrogen chloride? 2HCl →H₂ +Cl₂

When 0.01 mol of solid NaOH is added to 100 cm³ of 1.0 mol dm⁻³ HCl, the temperature increases by ∆T₁. What will be the temperature change, ∆T₂, for a second experiment in which the amount of NaOH and the volume of 1.0 mol dm⁻³ HCl are each doubled?

O₂(g) →2O(g) ∆H= 498 kJ 3O₂ (g) →2O ₃(g) ∆H= 284 kJ Using the information above, what is ∆H for the following equation in kJ?

The enthalpy changes for two reactions involving hydrogen are as follows: C(s) +2H₂ (g) →CH₄(g) ∆H = − 75 kJ H₂(g) →2H(g) ∆H = + 436 kJ What is the enthalpy change (in kJ) for the reaction CH₄ (g) →C(s) +4H(g) A. −947 B. +361 C. +511 D. +947

Consider the following reaction: N₂(g) +3H₂ (g) →2NH₃ (g) ∆H^θ=? Bond enthalpies (in kJ mol −1) involved in the reaction are N≡N x H–H y N–H z Which calculation will give the value of ∆H^θ?

Consider the following reactions: CH₃COOH +OH⁻→CH₃COO ⁻+H₂O ∆H^θ =q₁ kJ H⁺ +OH ⁻→H₂O ∆H^θ =q₂ kJ What is the enthalpy change for the reaction CH₃COOH →CH₃COO⁻ + H⁺

If 3600 J of heat is added to 180 g of C₂H₅OH(l), its temperature increases from 18.5^OC to 28.5^OC. What is the specific heat capacity of C₂H₅OH(l) in J/g/^OC ?

Using the information below: H₂(g) + O₂ (g) → H₂O₂ (l) ∆H = − 187.6 kJ 2H₂ (g) + O₂ (g) → 2H₂O(l) ∆H = − 571.6 kJ what is the value of ∆H (in kJ) for 2H₂O₂(l) → 2H₂O(l) + O₂(g)