Determine ?rH° for the following reaction, 2 NH3(g) + 5/2 O2(g) ? 2 NO(g) + 3 H2O(g). The thermochemical equations for the reaction are given below: \[\begin{array} { l l } \mathrm { N } _ { 2 } ( \mathrm {~g} ) + \mathrm { O } _ { 2 } ( \mathrm {~g} ) \rightarrow 2 \mathrm { NO } ( \mathrm { g } ) & \Delta _ { r } H ^ { \circ } = + 180.8 \mathrm {~kJ} / \text { mol-rxn } \\ \mathrm { N } _ { 2 } ( \mathrm {~g} ) + 3 \mathrm { H } _ { 2 } ( \mathrm {~g} ) \rightarrow 2 \mathrm { NH } _ { 3 } ( \mathrm {~g} ) & \Delta _ { r } H ^ { \circ } = - 91.8 \mathrm {~kJ} / \mathrm { mol } - \mathrm { rxn } \\ 2 \mathrm { H } _ { 2 } ( \mathrm {~g} ) + \mathrm { O } _ { 2 } ( \mathrm {~g} ) \rightarrow 2 \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { g } ) & \Delta _ { r } H ^ { \circ } = - 483.6 \mathrm {~kJ} / \mathrm { mol } - \mathrm { rxn } \end{array}\]

A) -1178.2 kJ/mol-rxn B) -452.8 kJ/mol-rxn C) -394.6 kJ/mol-rxn D) -211.0 kJ/mol-rxn E) +1178.2 kJ/mol-rxn A) -1178.2 kJ/mol-rxn B) -452.8 kJ/mol-rxn C) -394.6 kJ/mol-rxn D) -211.0 kJ/mol-rxn E) +1178.2 kJ/mol-rxn

The thermochemical equation for the combustion of methanol is given below. CH3OH( $\ell$ ) + 3/2 O2(g) ? CO2(g) + 2 H 2O(g) ?rH° = -638.7 kJ/mol-rxn What is the enthalpy change for the combustion of 8.59 g of CH3OH?

A) -171 kJ B) -19.9 kJ C) -2.38 × 103 kJ D) -5.49 × 103 kJ E) -1.76 × 106 kJ A) -171 kJ B) -19.9 kJ C) -2.38 × 103 kJ D) -5.49 × 103 kJ E) -1.76 × 106 kJ

What is the overall chemical equation that results from the sum of the given steps? 2 C(s) + 2 H2O(g) → 2 CO(g) + 2 H2(g) CO(g) + H2O(g) → CO2(g) + H2(g) CO(g) + 3 H2(g) → CH4(g) + H2O(g)

A) 2 C(s) + 2 H2O(g) → CO2(g) + CH4(g) B) 2 C(s) + 3 H2O(g) → CO(g) + CO2(g) + 3 H2(g) C) 2 C(s) + H2O(g) + H2(g)→ CO(g) + CH4(g) D) 2 CO(g) + 2 H2(g) → CH4(g) + CO2(g) E) 2 C(s) + CH4(g) + 3 H2O(g) → 3 CO(g) + 5 H2(g) A) 2 C(s) + 2 H2O(g) → CO2(g) + CH4(g) B) 2 C(s) + 3 H2O(g) → CO(g) + CO2(g) + 3 H2(g) C) 2 C(s) + H2O(g) + H2(g)→ CO(g) + CH4(g) D) 2 CO(g) + 2 H2(g) → CH4(g) + CO2(g) E) 2 C(s) + CH4(g) + 3 H2O(g) → 3 CO(g) + 5 H2(g)

Exam 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

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Acetylene, C₂H₂, is a gas used in welding. The molar enthalpy of combustion for acetylene is -2599 kJ. A mass of 0.338 g C₂H₂(g) is combusted in a bomb calorimeter. If the heat capacity of the calorimeter is 729 J/K and it contains 1.150 kg of water, what is the temperature increase of the bomb calorimeter? The specific heat capacity of water is 4.184 J/g⋅K and the molar mass of acetylene is 26.04 g/mol.

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Question 61

If 46.1 g of copper at 11.6 °C is placed in 85.0 g of water at 72.4 °C, what is the final temperature of the mixture? The specific heat capacities of copper and water are 0.385 J/g ⋅ K and 4.184 J/g ⋅ K, respectively.

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Question 62

When 50.0 mL of 1.60 M of HCl(aq) is combined with 50.0 mL of 1.70 M of NaOH(aq) in a coffee-cup calorimeter, the temperature of the solution increases by 10.7°C. What is the change in enthalpy for this balanced reaction? HCl(aq) + NaOH(aq) ? NaCl(aq) + H₂O( $\ell$ ) Assume that the solution density is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/g?°C.

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Question 63

Determine ?_rH° for the following reaction, 2 NH₃(g) + 5/2 O₂(g) ? 2 NO(g) + 3 H₂O(g). The thermochemical equations for the reaction are given below: ()+()\rightarrow2() =+180.8/ mol-rxn ()+3()\rightarrow2() =-91.8/- 2()+()\rightarrow2() =-483.6/-

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Question 64

When 10.0 g of KOH is dissolved in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 25.18 °C to 47.53 °C. What is the enthalpy change per gram of KOH dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/g ⋅ K.

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Question 65

The thermochemical equation for the combustion of methanol is given below. CH₃OH( $\ell$ ) + 3/2 O₂(g) ? CO₂(g) + 2 H ₂O(g) ?_rH° = -638.7 kJ/mol-rxn What is the enthalpy change for the combustion of 8.59 g of CH₃OH?

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Question 66

Which of the following thermodynamic quantities are state functions: heat (q), work (w), enthalpy change (ΔH), and/or internal energy change (ΔU)?

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Question 67

44.0 g of ice at -20.0 °C is mixed with 325 g of water at 32.1 °C. Calculate the final temperature of the mixture. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/g⋅K, liquid water = 4.184 J/g⋅K)

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Question 68

What is the overall chemical equation that results from the sum of the given steps? 2 C(s) + 2 H₂O(g) → 2 CO(g) + 2 H₂(g) CO(g) + H₂O(g) → CO₂(g) + H₂(g) CO(g) + 3 H₂(g) → CH₄(g) + H₂O(g)

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Question 69

Showing 61 - 69 of 69

If 46.1 g of copper at 11.6 °C is placed in 85.0 g of water at 72.4 °C, what is the final temperature of the mixture? The specific heat capacities of copper and water are 0.385 J/g ⋅ K and 4.184 J/g ⋅ K, respectively.

Determine ?_rH° for the following reaction, 2 NH₃(g) + 5/2 O₂(g) ? 2 NO(g) + 3 H₂O(g). The thermochemical equations for the reaction are given below: ()+()\rightarrow2() =+180.8/ mol-rxn ()+3()\rightarrow2() =-91.8/- 2()+()\rightarrow2() =-483.6/-

When 10.0 g of KOH is dissolved in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 25.18 °C to 47.53 °C. What is the enthalpy change per gram of KOH dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/g ⋅ K.

The thermochemical equation for the combustion of methanol is given below. CH₃OH( $\ell$ ) + 3/2 O₂(g) ? CO₂(g) + 2 H ₂O(g) ?_rH° = -638.7 kJ/mol-rxn What is the enthalpy change for the combustion of 8.59 g of CH₃OH?

Which of the following thermodynamic quantities are state functions: heat (q), work (w), enthalpy change (ΔH), and/or internal energy change (ΔU)?

44.0 g of ice at -20.0 °C is mixed with 325 g of water at 32.1 °C. Calculate the final temperature of the mixture. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/g⋅K, liquid water = 4.184 J/g⋅K)

What is the overall chemical equation that results from the sum of the given steps? 2 C(s) + 2 H₂O(g) → 2 CO(g) + 2 H₂(g) CO(g) + H₂O(g) → CO₂(g) + H₂(g) CO(g) + 3 H₂(g) → CH₄(g) + H₂O(g)

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Gases and Their Properties

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Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

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Principles of Chemical Reactivity: Entropy and Free Energy

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Exam 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

If 46.1 g of copper at 11.6 °C is placed in 85.0 g of water at 72.4 °C, what is the final temperature of the mixture? The specific heat capacities of copper and water are 0.385 J/g ⋅ K and 4.184 J/g ⋅ K, respectively.

Determine ?rH° for the following reaction, 2 NH3(g) + 5/2 O2(g) ? 2 NO(g) + 3 H2O(g). The thermochemical equations for the reaction are given below: ()+()\rightarrow2() =+180.8/ mol-rxn ()+3()\rightarrow2() =-91.8/- 2()+()\rightarrow2() =-483.6/-

When 10.0 g of KOH is dissolved in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 25.18 °C to 47.53 °C. What is the enthalpy change per gram of KOH dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/g ⋅ K.

The thermochemical equation for the combustion of methanol is given below. CH3OH( ℓ\ellℓ ) + 3/2 O2(g) ? CO2(g) + 2 H 2O(g) ?rH° = -638.7 kJ/mol-rxn What is the enthalpy change for the combustion of 8.59 g of CH3OH?

Which of the following thermodynamic quantities are state functions: heat (q), work (w), enthalpy change (ΔH), and/or internal energy change (ΔU)?

44.0 g of ice at -20.0 °C is mixed with 325 g of water at 32.1 °C. Calculate the final temperature of the mixture. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/g⋅K, liquid water = 4.184 J/g⋅K)

What is the overall chemical equation that results from the sum of the given steps? ​ 2 C(s) + 2 H2O(g) → 2 CO(g) + 2 H2(g) CO(g) + H2O(g) → CO2(g) + H2(g) CO(g) + 3 H2(g) → CH4(g) + H2O(g) ​

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

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Determine ?_rH° for the following reaction, 2 NH₃(g) + 5/2 O₂(g) ? 2 NO(g) + 3 H₂O(g). The thermochemical equations for the reaction are given below: ()+()\rightarrow2() =+180.8/ mol-rxn ()+3()\rightarrow2() =-91.8/- 2()+()\rightarrow2() =-483.6/-

The thermochemical equation for the combustion of methanol is given below. CH₃OH( $\ell$ ) + 3/2 O₂(g) ? CO₂(g) + 2 H ₂O(g) ?_rH° = -638.7 kJ/mol-rxn What is the enthalpy change for the combustion of 8.59 g of CH₃OH?

What is the overall chemical equation that results from the sum of the given steps? 2 C(s) + 2 H₂O(g) → 2 CO(g) + 2 H₂(g) CO(g) + H₂O(g) → CO₂(g) + H₂(g) CO(g) + 3 H₂(g) → CH₄(g) + H₂O(g)