Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Write a balanced formation equation determine the value of ΔHf° for the compound HCl (g)
- Write a balanced formation equation determine the value of ΔHf° for the compound NH3 (g).
- Write a balanced formation equation determine the value of ΔHf° for the compound SO3 (g)
- Write a balanced formation equation determine the value of ΔHf° for the compound CH3OH (l)
- Write a balanced formation equation determine the value of ΔHf° for the compound CaCO3 (s)
- Write a balanced formation equation determine the value of ΔHf° for the compound H2O (l)
- Write a balanced formation equation determine the value of ΔHf° for the compound NaCl (s)
- Write a balanced formation equation determine the value of ΔHf° for the compound NO (g)
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- A chemist measures the enthalpy change ΔH during the following reaction: 2Al(OH)3(s)→Al2O3(s)+ 3H2O(l) ΔH=41.kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔH Al2O3(s) + 3H2O(l) → 2Al(OH)3(s) kJ 3Al2O3(s) + 9H2O(l) → 6Al(OH)3(s) kJ 4Al(OH)3(s)+2Al2O3(s) + 6H2O(l) kJarrow_forwardConsider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l) ΔH1HA(aq) → H+(aq) + A-(aq) ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l) ΔH3Choose the equation that shows the correct relationship between their enthalpy changes. A.) ΔH1 = ΔH3 - ΔH2 B.) ΔH2 = ΔH1 + ΔH3arrow_forwardPart O Which reactions are exothermic? Reaction 1: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) + 2220 kJ Reaction 2: 4 H2(g) + 2 O2(g) → 4 H2O(l) + 1140 kJ Reaction 3: 2 H2O(l) + 88 kJ → 2 H2(g) + O2(g) Reaction 3 Reactions 2 and 3 Reaction 1 and 2 All reactions are since they produce products.arrow_forward
- Which of the following represents an endothermic reaction? O CH4 (g) + 202 (g) → CO2 (g) + 2H2O (g) + 890 kJ 2S02 (g) 25 (s) + 20, (g) + 376kJ O 2C2H6 (g) + 702 (g) → 4CO2 (g) + 6H2O(g) + 3120 kJ 2H20 (g) + 572 kJ → 2H2 (g) + O2 (g)arrow_forwardA cold pack contains 134.4 g of water and 40.7 g of ammonium nitrate. What will be the final temperature of the activated cold pack, if the initial temperature is 26.8 °C? (Assume that the specific heat of the solution is the same as that for water, 4.184 J/g °C and no heat is lost). The heat of solution of ammonium nitrate is 25.4 kJ/mol. Please do not include units in your answer.arrow_forwardConsider these reactions: Reaction 1: H₂(g) + Cl₂(g) → 2HCl(g) Reaction 2: 20F₂ (g) → O₂(g) + 2 F₂ (g) Reaction 3: N₂(g) + 2O₂(g) → 2NO₂ (9) Use Reaction 1. AH = -184.6 kJ AH = -49.4 kJ AH = +66.4 kJ Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,861.0 kJ of energy is released from the system. Round to the nearest whole number. Answer:____ garrow_forward
- 4. The specific heat of water is quite high at 4.184 J/gC. Explain how life on this planet would be different if the specific heat of water were that of lead at 0.128 J/gC.arrow_forwardConsider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l) ΔH1HA(aq) → H+(aq) + A-(aq) ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l) ΔH3Choose the equation that shows the correct relationship between their enthalpy changes.arrow_forwardThe standard enthalpy change for the following reaction is 103 kJ at 298 K. N2(g) + O2(g) + Cl2(g) ---------> 2 NOCl(g) ΔH° = 103 kJ What is the standard enthalpy change for this reaction at 298 K? 1/2 N2(g) + 1/2 O2(g) + 1/2 Cl2(g)--------> NOCl(g) kJarrow_forward
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