The enthalpy changes for three compounds are shown below: N2(g) + 5/2 O2(g) + 15.0 kJ H2(g) + 1/2 02(g) 1/2 H2(g) + 1/2 N2(g) + 3/2 02(g) N₂O5(8) H₂O(1) + 285.8 kJ A/ HNO3(1) + 174.1 kJ Net: N₂O5(g) + H₂O (1) 2 HNO3(1) The standard enthalpy change for the net reaction is: ab.c kJ Input the value for ab.c in the blank below. Include a positive or negative sign in your answer: eg -16.8 or +16.8 • Do not include units Is the reaction endothermic or exothermic? • write exothermic or endothermic in the blank

The enthalpy changes for three compounds are shown below: N2(g) + 5/2 O2(g) + 15.0 kJ H2(g) + 1/2 02(g) 1/2 H2(g) + 1/2 N2(g) + 3/2 02(g) N₂O5(8) H₂O(1) + 285.8 kJ A/ HNO3(1) + 174.1 kJ Net: N₂O5(g) + H₂O (1) 2 HNO3(1) The standard enthalpy change for the net reaction is: ab.c kJ Input the value for ab.c in the blank below. Include a positive or negative sign in your answer: eg -16.8 or +16.8 • Do not include units Is the reaction endothermic or exothermic? • write exothermic or endothermic in the blank

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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Coffee cup calorimetry was used to determine the enthalpy of solution of lithium iodide (LiI): A) First, the coffee cup was calibrated. 50.0 mL of water (s=4.184J/g×0 C) was heated to 95.50C and mixed with 50.0 mL of cool water at 22.30 C. The temperature of the contents of the coffee cup stabilized at 49.40 C. Determine the heat capacity of the coffee cup. B) Next, the enthalpy of solution of lithium iodide (LiI) was determined. 0.0g of solid lithium iodide was added to 100mL of water at 23.20 C in the coffee cup, and the temperature increased to 32.10 C. Calculate the enthalpy of the solution of lithium iodide.
The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is qH2O?
How many litres of C6H14(l)C6H14(l), measured at 20 ∘C, must be burned to provide enough heat to warm 26.4 m^3of water from 18.2 to 33.1 ∘C , assuming that all the heat of combustion is transferred to the water, which has a specific heat of 4.18 J g^−1 ∘C? Recall that 1 mL=10−3 L1 mL=10−3 L. Express your answer to four significant figures and include the appropriate units.
Calculate the enthalpy change for the following reaction, _C₂H4 (9) + using the following standard heats of formation: AH(C₂H4) = +52.5 kJ/mol; AH(CF4) =-933.0 kJ/mol; AH (HF) =-271.6 kJ/mol _F₂(g) → _CF4(g) + _HF(g)
Use standard enthalpies to determine the enthalpy change from the following reaction occurring: (1:3) 2Cl₂(g) + 2H₂O(g) →4HCl(g) + O₂(g)
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1.Given reactions A - C, determine the the change in enthalpy (kJ) for the reaction between C(s) + H2(g). Do not type units into your answer. C(graphite) + 2 H2(g) ⟶⟶ CH4(g) Δ?=?ΔH=? A. C(graphite) + O2(g) ⟶⟶ CO2(g) Δ?=−393.51??ΔH=−393.51kJB. H2(g) + 1/2 O2(g) ⟶⟶ H2O(l) Δ?=−285.83??ΔH=−285.83kJC. CO2(g) + 2 H2O(l) ⟶⟶ CH4(g) + 2 O2(g) Δ?=890.30??ΔH=890.30kJ 2. Based on your answer to the previous problem, determine the value of q (kJ) if 5.08 grams of methane (CH4) gas is produced from graphite and hydrogen gas. Do not type units into your answer.
Help with number 3 please
Use Hess’s law to obtain the enthalpy change for this reaction: H2(g) + 1/8 S8(rhombic) -> H2S(g) from the following enthalpies:H2S(g) + 3/2 O2(g) à H2O(g) + SO2(g) ΔH = -518 KJH2(g) + ½ O2(g) à H2O(g) ΔH = -242 KJ1/8 S8(rhombic) + O2(g) à SO2(g) ΔH = -297 KJ
1) From the following data, C(graphite) + O2(g) à CO2(g) = -393.5 kJ/mol H2(g) + 1/2O2(g) = H2O(l) delta H = -285.8 kJ/mol 2C2H6(g) + 7O2(g) = 4CO2(g) + 6H2O(l) delta H = -3119.6 kJ/mol calculate the enthalpy change for the reaction 2C(graphite) + 3H2(g) =C2H6(g) a) –2417.2 kJ b) –84.6 kJ c) 2417.2 kJ d) –3204.2 kJ
Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H₂(g) C4H10(9) (2) C₂H4(g) →→2C(s) + 2H₂(g) (3) 2C₂H4(g) + H₂(g) C4H10 (9) ΔΗ° = -125.6 kJ what is the standard enthalpy change for the reaction: KJ AHO = -52.3 kJ ΔΗ° = ?
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?