9.98. Hydrogen combines with oxygen in fuel cells according to the thermochemical equation 2 H2 (g) + O2 (g) → 2 H2O(g) AH° = -571.7 kJ Suppose that you are working with a firm that is using hydrogen fuel cells to power satellites. The satellite requires 4.0 × 10 kJ of energy during its useful lifetime to stabilize its orbit. Describe how you would determine the mass of hydrogen you would need in your fuel cells for this particular satellite.

9.98. Hydrogen combines with oxygen in fuel cells according to the thermochemical equation 2 H2 (g) + O2 (g) → 2 H2O(g) AH° = -571.7 kJ Suppose that you are working with a firm that is using hydrogen fuel cells to power satellites. The satellite requires 4.0 × 10 kJ of energy during its useful lifetime to stabilize its orbit. Describe how you would determine the mass of hydrogen you would need in your fuel cells for this particular satellite.

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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3. Sodium reacts violently with water to form sodium hydroxide as shown in the following equation: 2Na(s) + 2H₂O → 2NaOH(aq) + H₂(g) A 0.37 g piece of sodium is placed in 175.0 g of water. The water temperature increased from 19.30 °C to 25.70 °C. Determine the molar enthalpy of the reaction. (Enthalpy per mole of sodium)
Part of the industrial recovery of elemental zinc from the zinc sulfide ore is by roasting: ZnS) + O2(2) → ZnOs + SO22) AH = -879 kJ/mol Calculate the amount of heat (in kJ) released when 1.00 g of zinc sulfide reacts with excess oxygen.
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
In a coffee cup calorimeter, 50.0 mL of 0.124 M AgNO3 and 50.0 mL of 0.124 M HBr are mixed. The following reaction occurs. Ag*(aq) + Br (aq) → AgBr(s) If the two solutions are initially at 23.92°C, and if the final temperature is 25.17°C, calculate AH for the reaction in kJ/mol of AgBr formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of 4.18 J °C-1g-¹. kJ/mol
One day while camping, a student used a propane stove to boil some water. The student heated 5.00 L of water from 15.6°C to 98.5°C. The molar enthalpy of combustion of propane is -2043.9 kJ/mol and heating the water required 1.38 mol of propane. Determine the efficiency of the propane camp stove if the heat released from the stove was used to heat the water. 62.4 % 38.4% D162 % 61.6%
Copper has been used for thousands of years, either as a pure metal or in alloys. It is frequently used today in the production of wires and cables. Copper can be obtained through smelting or recycling. Determine the energy associated with each of these processes in order to recycle 1.40 mol Cu. The smelting of copper occurs by the balanced chemical equation: CuO(s) +CO(g) → Cu(s) +CO,(g) where AHtCuo is = - 155 kJ/mol. Assume the process of recycling copper is simplified to just the melting of the solid Cu starting at 25°C. The melting point of Cu is 1084.5°C with AH®fus = 13.0 kJ/mol and a molar heat capacity, CPCU = 24.5 J/mol:°C.
Consider the combustion of liquid C₅H₈ in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of C₅H₈ is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.634 °C. What quantity in moles of C₅H₈ were burned?
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A chemist measures the enthalpy change AH during the following reaction: 2 Al(OH),(s)-Al,0,(s) + 3H,0(1) AH=41. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ 3AI,0,(s) + 9H,0() 6Al(OH),(s) Al,0,(s) + 3H,0() 2Al (OH), (s) Al(OH),(6) - Al,0,(0) + ,00 1 Al,0,(5) + H,0() O kJ Explanation Check 2021 McGra M B
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Using Hess's Law to calculate net reaction enthalpy Dwayne The lead-acid storage battery is the oldest rechargeable battery in existence. It was invented in 1859 by French physician Gaston Plante and still retains application today, more than 150 years later. There are two reactions that take place during discharge of the lead-acid storage battery. In one step, sulfuric acid decomposes to form sulfur trioxide and water: H, SO (1) SO,(g) + II,0(1) AH= +113. kJ 圖 In another step, lead, lead(IV) oxide, and sulfur trioxide react to form lead(II) sulfate: alo Pb(1+ PbO,(s) + 2 SO,(g) 2 PbSO (s) AH = -775. kJ Calculate the net change in enthalpy for the formation of one mole of lead(II) sulfate from lead, lead(IV) oxide, and sulfuric acid from these reactions. Round your answer to the nearest kJ. OKT Explanation Check O 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility 5:03 AM ENG 39°F Clear 12/14/2021 P Type here to search
In a coffee cup calorimeter, 3.00 g of NaOH (molar mass 40.00g/mol) was mixed with 75.0 mL of 1.00M HNO3. If the initial temperature of the HNO3 was 31.3°C and the final temperature of the solution was 22.3°C, determine AH for the reaction in kJ/mol. NaOH(s) + HNO3(aq) ===> NaNO3(aq) + H2O) The density and the specific heat capacity of the resulting solution are 1.00 g/ml and 4.18 J/°C.g, respectively. Units do not need to be typed, simply enter the correct number. If the sign of AH is negative put a negative sign (-) in the answer. Answer: