Be sure to answer all parts.When organic matter decomposes under oxygen-free (anaerobic) conditions, methane is one of theproducts. Thus, enormous deposits of natural gas, which is almost entirely methane, serve as a majorsource of fuel for home and industry.(a) Known deposits of natural gas can produce 5,400 EJ of energy (1 EJ = 10¹8 J). Current totalglobal energy usage is 3.9 × 102 EJ per year. Find the mass (in kg) of known deposits of natural gas (A0H for the combustion of CH4 = -802 kJ/mol).rxnx 10kg CH4(b) At current rates of usage, for how many years could these deposits supply the world's total energyneeds?yr(c) What volume (in ft³) of natural gas, measured at STP, is required to heat 1.00 qt of water from25.0°C to 59.1°C (d of H₂O = 1.00 g/mL; d of CH4 at STP = 0.72 g/L)?ft³(d) The fission of 1 mol of uranium (about 4 x 10-4 ft³) in a nuclear reactor produces 2 × 10¹3 J.What volume (in ft) of natural gas would produce the same amount of energy?x 10

Given: Energy produced from natural gas=5,400 EJ=5,400×1018 J 1 EJ =1018…

When organic matter decomposes under oxygen-free (anaerobic) conditions, methane is one of the products. Thus, enormous deposits of natural gas, which is almost entirely methane, serve as a major source of fuel for home and industry. (a) Known deposits of natural gas can produce 5,400 EJ of energy (1 EJ = 10¹8 J). Current total global energy usage is 3.9 x 102 EJ per year. Find the mass (in kg) of known deposits of natural gas (A H for the combustion of CH4-802 kJ/mol). rxn x 10 kg CH4 (b) At current rates of usage, for how many years could these deposits supply the world's total energy needs? yr (c) What volume (in ft³) of natural gas, measured at STP, is required to heat 1.00 qt of water from 25.0°C to 59.1°C (d of H₂O-1.00 g/mL; d of CH4 at STP=0.72 g/L)? ft³ (d) The fission of 1 mol of uranium (about 4 x 10-4 ft) in a nuclear reaftor produces 2 x 10¹3 J. What volume (in ft) of natural gas would produce the same amount of energy? x 10

When organic matter decomposes under oxygen-free (anaerobic) conditions, methane is one of the products. Thus, enormous deposits of natural gas, which is almost entirely methane, serve as a major source of fuel for home and industry. (a) Known deposits of natural gas can produce 5,400 EJ of energy (1 EJ = 10¹8 J). Current total global energy usage is 3.9 x 102 EJ per year. Find the mass (in kg) of known deposits of natural gas (A H for the combustion of CH4-802 kJ/mol). rxn x 10 kg CH4 (b) At current rates of usage, for how many years could these deposits supply the world's total energy needs? yr (c) What volume (in ft³) of natural gas, measured at STP, is required to heat 1.00 qt of water from 25.0°C to 59.1°C (d of H₂O-1.00 g/mL; d of CH4 at STP=0.72 g/L)? ft³ (d) The fission of 1 mol of uranium (about 4 x 10-4 ft) in a nuclear reaftor produces 2 x 10¹3 J. What volume (in ft) of natural gas would produce the same amount of energy? x 10

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...

See similar textbooks

Related questions

Q: Calculate the kinetic energy in joules of an automobile weighing 4175 lb and traveling at 45 mph. (1…

Q: Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in the form of…

A: According to the given reaction, 393.5 kJ of heat is produced on the formation of one mole of carbon…

Q: When organic matter decomposes under oxygen-free (anaerobic) conditions, methane is one of the…

A: a) Given that : Energy E = 5600 EJ = 5600×1018 J ΔH°rxn for the combustion of CH4 = -802kJ/mol =…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.65 kg sample…

Q: The reaction of hydrogen and nitrogen gases produces 5.00 g of ammonia and releases 3250 cal of…

Q: An unknown sample of coal is burned in an apparatus with a calorimeter constant of 0.96 kJ/°C. When…

Q: A student places 125g of liquid water, H201), at 24 °C into a coffee-cup calorimeter, and then adds…

A: Here the system is showing two change , one is the dissolution of KBr and another one is for…

Q: A 1753 kg1753 kg car is traveling down the road at 82.2 km/h.82.2 km/h. While traveling at this rate…

Q: Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions…

A: The balanced reaction taking place is given as, 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)…

Q: A 50.0 g sample of scandium, Sc, is heated by exposure to 1.50 x 10J. The temperature of the Sc is…

A: Given: Mass of water = 50.0 g Heat energy = 1.50×10 J Change in temperature = 61.1 oC

Q: The change in enthalpy (heat of solution) for ammonium nitrate dissolving in water is 25.7 kJ/mol.…

A: Given, The change in enthalpy (heat of solution) for ammonium nitrate dissolving in water is 25.7…

Q: The change in enthalpy (heat of solution) for ammonium nitrate dissolving in water is 25.7 kJ/mol.…

A: Molar mass of ammonium nitrate =80.043g/mol

Q: A piece of cobalt originally at 90.6°C was placed into a coffee cup calorimeter containing 200.0…

Q: Calculate the heat of reaction in joules. Assume that the specific heats of all solutions are 4.18…

Q: Using the partial equations below, determine the enthalpy of formation of nitric oxide (NO). Hint:…

Q: Consider the following reaction A(s) → B(s)+ C(g) AH= 80. 89 kJ/mol (a) What is AH for the reverse…

A: a= Δ H =-80.89 unit = kJ as in reverse direction only the sign changes b.for 1 mol it is…

Q: 8. The caloric content of some pasta (listed on the side of the box of pasta!) is 4.000 kcal per…

A: The amount of heat required to increase the temperature of one kilo gram of a substance by one…

Q: A chemist placed a 1.195 g sample of fuel in a bomb calorimeter which was immersed into 2.00 L of…

A: The mass of the fuel sample is = 1.195 g The increase in the temperature of the water is = 20.1oC to…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 196.0 g sample…

Q: chemical reaction has a negative enthalpy of reaction (-ΔHrxn) What does this tell you about the…

A: We have to find which option is correct

Q: Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in the form of…

Q: 12. An aluminum kettle weighs 1.05 kg.(a) What is the heat capacity of the kettle?(b) How much heat…

A: (a) Given that mass of aluminium kettle =1.05 kg = 1050 g Now, heat capacity is explained as the…

Q: Coal power plants burn large amounts of coal, C(s), in an O2(g) atmosphere to generate electricity.…

A: For the reaction., C(s) + O2(g) -------> CO2(g) Mass of carbon burnt = 102 metric tons Oxygen…

Q: What is the heat capacity of 265 grams of water? The specific heat of water is 4.184 J/g °C.

A: • The values provided in the question are:- i) Mass of water, m = 265 g ii) Specific heat capacity…

Q: What is the energy of system A? What is the energy of system B? In how many ways can the energy of…

A: we have given the two diagrams showing the energies (boxes) of each of four A particles and four B…

Q: A student heats 62.33 grams of chromium to 99.36 °C and then drops it into a cup containing 82.16…

A: Given, mass of chromium =62.33 graminitial temperature of chromium =99.36 °Cmass of water =82.16…

Q: A piece of metal with a specific heat of 1.09 J/gºC is heated to 108ºC and then placed in 139.785 g…

A: Given that: Mass of water = 139.785 gInitial temperature of water = 1.7oCFinal temperate of water…

Q: propane (C:H8) produces 2220 kJ of = consumed. What mass in grams of eat 55.0 gal of bathtub water…

A: According to the question, the combustion of propane will produce 2220 kJ of energy per mole. We…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.29 kg sample…

A: 0.45 or 4.49 * 10-1 J/g K

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.85 kg sample…

Q: Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HC1(aq) 2 MCI, (aq) + 3…

Q: A calorimeter holds 50 g water at 29.0°C. A sample of hot iron is added to the water, and the final…

Q: absorbs 1.357E3 J of heat. The final temperature of the sand is 6.7E1 °C. What is the mass (in g) of…

A: Given: Initial temperature = 2.24E1 Â°C Final temperature = 6.7E1 Â°C Amount of heat absorbed =…

Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

Be sure to answer all parts.
When organic matter decomposes under oxygen-free (anaerobic) conditions, methane is one of the
products. Thus, enormous deposits of natural gas, which is almost entirely methane, serve as a major
source of fuel for home and industry.
(a) Known deposits of natural gas can produce 5,400 EJ of energy (1 EJ = 10¹8 J). Current total
global energy usage is 3.9 × 102 EJ per year. Find the mass (in kg) of known deposits of natural gas (A
0
H for the combustion of CH4 = -802 kJ/mol).
rxn
x 10
kg CH4
(b) At current rates of usage, for how many years could these deposits supply the world's total energy
needs?
yr
(c) What volume (in ft³) of natural gas, measured at STP, is required to heat 1.00 qt of water from
25.0°C to 59.1°C (d of H₂O = 1.00 g/mL; d of CH4 at STP = 0.72 g/L)?
ft³
(d) The fission of 1 mol of uranium (about 4 x 10-4 ft³) in a nuclear reactor produces 2 × 10¹3 J.
What volume (in ft) of natural gas would produce the same amount of energy?
x 10

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

An unknown sample of coal is burned in an apparatus with a calorimeter constant of 0.72 kJ/°C. When a 0.329-g sample is used, the temperature change is 8.49°C. What is the energy density of the sample in kJ/g? Round your answer to 2 decimal places.
Constants | Periodic Table Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: Part B AHm = En,AH: (products)- E n,AH (reactants) For the reaction given in Part A. how much heat is absorbed when 3.50 mol of A reacts? where n represents the stoichiometric coefficients. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) Value Units Submit Previous Answers X Incorrect; Try Again; 29 attempts remaining Provide Feedback Pearson O 1:35 21
A gas expands and does work on the surroundings equal to 3.55 L atm. At the same time, it releases 540.4 J of heat to the surroundings. What is the change in energy in J of the gas? (write the solution without decimals)
The sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area (1 watt = 1 J/s). The plants in an agricultural field produce the equivalent of 23 kg of sucrose (C12H22 O11) per hour per hectare (1 ha = 10,000 m²). Assuming that sucrose is produced by the reaction 12CO₂(g) + 11H₂O(l) → C12H22 O11 (8) + 1202 (9) AH = 5640 kJ calculate the percentage of sunlight used to produce the sucrose - that is, determine the efficiency of photosynthesis in this field. Percent efficiency = %
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
59.) Gasohol is gasoline mixed with ethanol (C2H5OH). If 0.230 g of ethanol produces 7.24 kJ of energy when burned, what would be the AH for the combustion of one mole of ethanol?
2. A piece of Cu metal is heated in a test until the temperature reaches 96 °C and dropped into a calorimeter with 50.0 ml of water with a temperature of 27°C. after the addition of the metal, temperature of water in the calorimeter rises to 29 °C What is the mass of Cu added?
1 A piece of metal with a specific heat of 1.011 J/gºC is heated to 123.1ºC and then placed in 111.031 g of water which is at a temperature of 3.6 ºC. After a minute, the temperature of the water has stopped changing and is now 55.8ºC. Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/gºC. Enter your answer with at least 3 sig figs.
Which of the reactions are exothermic? 2 Mg(s) + O,(g) → 2 MgO(s) + heat O NH, (g) + HCI(g) → NH,CI(s) + heat AgCl(s) + heat – Ag*(aq) + Cl¯(aq) 2 Fe, 0, (s) + 3 C(s) + heat → 4Fe(s) + 3 CO, (g) O C(graphite) + 0,(g) → CO,(g) + heat O CH, (g) + 20,(g) → CO,(g) + 2 H,O(1) + heat
Suppose that the total mass of the reactants in a chemical reaction was 100.00000 g. How many kilojoules of energy would have to evolve from this reaction if the total mass of the products could be no greater than 99.99900 g? 9E7 kJ If all this energy were used to heat water, how many liters of water could have its temperature raised form 21.4°C to 96.8°C?
A gas expands and does work on the surroundings equal to 4.92 Latm. At the same time, it releases 98.6 J of heat to the surroundings. What is the change in energy in J of the gas? (write the solution without decimals)
An unknown sample of coal is burned in an apparatus with a calorimeter constant of 0.73 kj/°c. When a 0.26-g sample is used, the temperature change is 10.5°C. What is the energy density of the sample in k/g? Round your answer to 2 decimal places.