Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in the form of charcoal) to produce 4.90 kJ × 10² kJ of heat? The balanced chemical equation is as follows: C(s) + O2 (g) → CO2 (g), ΔΗ -393.5 kJ Express the mass in grams to three significant figures. ο ΑΣφ т 3

Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in the form of charcoal) to produce 4.90 kJ × 10² kJ of heat? The balanced chemical equation is as follows: C(s) + O2 (g) → CO2 (g), ΔΗ -393.5 kJ Express the mass in grams to three significant figures. ο ΑΣφ т 3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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CHEMISTRY (Please write the complete solution legibly. Choose the correct answer. No long explanation needed. Answer in 2 decimal places. Box the final answer.) The combustion of ammonia with oxygen occurs by the reaction: 4NH3(g) + 7O2(g) → 4NO2(g) + 6H2O(g) ΔH° = –1132 kJCalculate the amount of heat released when 2.00 gram of NH3 is combusted. a) 33.2 kJ b) 87.0 kJ c) 11.4 kJ d) 16.6 kJ
Do the follow reactions depict Heat of Formation Reactions? If so, mark the reaction as YES, if it is not a Heat of Formation Reaction, then choose NO. ✓3/2 H₂(g) + P(s) → PH3(g) H₂(g) + 1/2O₂(g) → H₂O(g) Al(s) + 3/2 Br₂(1)→ AlBr3(S) Na(s) + H₂O(1)→ NaOH(aq) + 1/2 H₂(g) ✓2As(s) + 5/2 O₂(g) → As2O5(s) In formation reactions the reactants must be elements in their most common states, and the only product is one mole of the substance of interest.
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 3.50 kg of water at 38.6 °C. During the reaction 131. kJ of heat flows out of the flask and into the bath.Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18·J·g^−1K^−1. Round your answer to 3 significant digits.
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCI(aq) 2 MCI, (аq) + 3 Н, (2) AH1 = -556.0 kJ 2. HCl(g) HCl(aq) AĦ2 = -74.8 kJ 3. H, (g) + Cl, (g) → 2 HCI(g) ΔΗ = -1845.0 kJ 4. MCI, (s) – MCI, (aq) AĦ4 = -493.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) – - 2 MCl, (s) -556.0 ΔΗ- Incorrect
Explain what the equation Q = m•C•ΔT means and how it relates to energy and calorimetry.
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 2.70kg of water at 39.2°C . During the reaction 128.kJ of heat flows out of the bath and into the flask. Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18·J·g−1K−1 . Be sure your answer has the correct number of significant digits.
When 145 mL of 0.212 M NaCl(aq) and 145 mL of 0.212 M AgNO3(aq), both at 21.1°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.7°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 3.14 ✕ 103 J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g·°C, and 0.997 g/mL, respectively). Using this data, calculate ΔH in kJ/mol of AgNO3(aq) for the given reaction.
According to the following reaction, how many grams of hydrogen would be needed to produce 5.450 x 103 kJ of energy? Assume excess oxygen. Do not type units into your answer. H2(g) + 1/2 O2(g) ⟶⟶ H2O(l) Δ?=−285.83??ΔH=−285.83kJ
A chemical reaction takes place inside a flask submerged in a water bath. The water bath contains 9.10 kg of water at 34.3°C. During the reaction 62.1 kJ of heat flows out of the bath and into the flask.Calculate the new temperature of the water bath. You can assume the specific heat capacity of water under these conditions is 4.18·J·g−1K−1. Round your answer to 3 significant digits.
Consider the following reaction. (a) Is the reaction exothermic or endothermic? exothermic endothermic CH3OH(g) → CO(g) + 2 H₂(g) AH +90.7 kJ (b) Calculate the amount of heat transferred when 35.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. ΔΗ= 100.8 (c) If the enthalpy change is 19.0 kJ, how many grams of hydrogen gas are produced? 0.42 x g (d) How many kilojoules of heat are released when 13.0 g of CO(g) reacts completely with H₂(g) to form CH₂OH(g) at constant pressure? AH = -90.7 X kJ (e) Calculate AE when 400.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol K-41.7 XkJ HopHelpCh5N1
4. You wish to determine the amount of heat produced by the reaction of propane with oxygen. You are given some known reactions: I. II. III. 3 C(s) (g) + 4H₂(g) → C₂H₂ (g) C(s) (g) + O₂(g) → CO₂ (g) H₂(g) + O₂(g) → H₂O (1) ΔΗ, ΔΗ, ΔΗ, (a) Combine reactions 1, 2 and 3 to form a series of steps that sum to the combustion of propane: C₂H₂(g) +50₂ (g) →3CO₂ (g) + 4H₂O (1) (b) Given the following values for the enthalpy changes, combustion of propane. AH₂=-393.5 kJ/mol AH, =-103.85 kJ/mol calculate AH for the AH, = -285.8kJ/mol
Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCl(aq) → 2 MCI, (aq) + 3 H, (g) AH = -931.0 kJ HCI(g) → HCI(aq) AH2 = -74.8 kJ H,(g) + Cl,(g) → 2 HCI(g) AH3 = -1845.0 kJ 4. MCI, (s) → MCI, (aq) AH, = -118.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) → 2 MCI, (s) 2. 3.