On a 5 day wilderness expedition you'll need to heat 3.0 kg of water to the boiling point each day. The air temperature will average 25 °C. You have availablecanisters of compressed propane (C3H8) fuel, which you'll burn to heat the water. Each canister has 25. g of propane in it. What is the minimum number of fuelcanisters you must bring?The standard heat of formation of propane at 25 °C is -103.8 kJ/mol. You'll probably find other helpful data in the ALEKS Data resource.canisters:13XG000Ar

Since you cannot have a fraction of a canister, you will need 80 canisters. Final Answer:You must…

Answered: On a 5 day wilderness expedition you'll…

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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On a 10 day wilderness expedition you'll need to heat 5.0 kg of water to the boiling point each day. The air temperature will average 25 °C. You have available canisters of compressed butane (C,H10) fuel, which you'll burn to heat the water. Each canister has 100. g of butane in it. What is the minimum number of fuel canisters you must bring? The standard heat of formation of butane at 25 °C is – 125.7 kJ/mol. You'll probably find other helpful data in the ALEKS Data resource. canisters:
On a 7 day wilderness expedition you'll need to heat 2.0 kg of water to the boiling point each day. The air temperature will average 25 °C. You have available canisters of compressed propane (C,H) fuel, which you'll burn to heat the water. Each canister has 25. g of propane in it. What is the minimum number of fuel canisters you must bring? The standard heat of formation of propane at 25 °C is – 103.85 kJ/mol. You'll probably find other helpful data in the ALEKS Data resource. canisters:
2 A student determines the heat of dissolution of solid cobalt(II) sulfate using a coffee-cup calorimeter of negligible heat capacity. When 1.34 g of CoSO4(s) is dissolved in 101.00 g of water, the temperature of the solution increases from 25.00 to 26.69 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoSO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.
THe G.R.A.S.P. method
In a coffee cup calorimeter, 40.0 mL of 0.33 M nitric acid (HNO3) and 40.0 mL of 0.33 M potassium hydroxide (KOH) are mixed to observe the heat released during the neutralization reaction. Based on the data in the table, what is the enthalpy of the neutralization reaction between HNO3 and KOH? Initial temperature in the calorimeter (°C) Final temperature in the calorimeter (°C) Final mass of the neutralized solution (g) Calorimeter constant (J/C)) 21.3 23.5 79.74 4.57
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C. The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data. Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol). C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy
Chemistry 14) A 60.0 mL quantity of 0.80 M HCI is mixed with 60.0 mL of 0.80 M KOH in a constant pressure calorimeter with negligible heat capacity. If the initial temperatures of both solutions are equal to 20.24°C. Calculate the heat change of the neutralization reaction if the final temperature of the mixture is 30.0°C. Assume that the densities and specific heats of the solutions are the same as those of water (1.00 g/mL and 4.184 J/g °C, respectively). Note: this point is worth 10 points. A) + 4900.3 J B)-1171.2 J C)-2450.15 J D)-4900.3 J
When a 4.31 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.3 °C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.2 kJ/•C. The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane. Enter your answer numerically and in terms of kJ/mol.
A 3.000 g sample of food was then burned in a calorimeter to determine its Calories per gram content. 50mL of water were used to determine ΔT of the reaction. Initial temperature of the water at the start of the combustion reaction was 20oC, final temperature was 99oC. Calorimeter constant for this calorimeter is 10.0J/oC. How much heat has been absorbed by the water sample?
1. Magnesium solid reacts with aqueous hydrochloric acid to form the Mg2+ ion in solution. In an experiment, 60.0 mL of aqueous HCl was mixed with 0.1297 g of magnesium solid in a double Styrofoam cup calorimeter. The reaction caused the temperature of the substances in the calorimeter to rise 10.02°C. Assume the density and specific heat of the HCl solution is that of water, 1.00 g/mL and 4.184 J/g °C, respectively. The specific heat of magnesium is 1.02 J/g °C. a. Write the balanced chemical equation for this reaction. b. Calculate the heat of this reaction, AHrxn, in kJ. c. Calculate the heat of this reaction per mole of Mg2+ formed, AHxn/mole Mg²+. d. The literature value of this reaction is -466.85 kJ/mole. Calculate the percent deviation of the experimental value from the literature value.
In an experiment, a 0.5002 g sample of tridecanedioic acid ( C13 H24 O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.165 × 10³ g of water. During the combustion the temperature increases from 21.99 to 24.52 °C. The heat capacity of water is 4.184 J·g¯¹. °C-¹. The heat capacity of the calorimeter was determined in a previous experiment to be 904.0 J. °C¯¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of tridecanedioic acid based on these data. C13H24 O4(s) + 17O2 (g) → 12H₂O(l) + 13CO2 (g) + Energy kJ/mol Molar Heat of Combustion =
On a 14 day wilderness expedition you'll need to heat 3.0 kg of water to the boiling point each day. The air temperature will average 25 °C. You have available canisters of compressed propane (C₂Hg) fuel, which you'll burn to heat the water. Each canister has 50. g of propane in it. What is the minimum number of fuel canisters you must bring? The standard heat of formation of propane at 25 °C is -103.8 kJ/mol. You'll probably find other helpful data in the ALEKS Data resource. canisters: 0 X Ś

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