On a 10 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 h available canisters of compressed butane (C4H₁o) 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: X S

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A quantity of 2.00×102 mL of 0.786 M HCl is mixed with 2.00×102 mL of 0.393 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.76°C. For the process below, the heat of neutralization is −56.2 kJ/mol. What is the final temperature of the mixed solutions?   H+(aq) + OH−(aq)→H2O(l)   _____°C

In Part B of the experiment, a student mixes 30.0 mL of 1.1 M HC1(aq) with 30.0 mL of 1.000 M NaOH(aq) in a well-insultated calorimeter and observes that the temperature of the solution increases by 5.75 °C. These are similar conditions as the previous two problems. How many moles of water are formed? number of moles of water = mol

A 100.0-mL sample of 1.0 M NaOH is mixed with 50.0 mL of 1.0 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing is 22.3 °C. After the NaOH solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured is 31.4 °C. Assume that the density of the mixed solution is 1.00 g/mL, the specific heat of the mixed solutions is 4.18 J/g•°C, and no heat is lost to the surroundings.(a) Write a balanced chemical equation for the reaction that takes place.(b) Is there any unreacted NaOH or H2SO4 remaining after the reaction?(c) Calculate the enthalpy change per mole of H2SO4 in the reaction.

At constant volume, the heat of combustion of a particular compound is -3916.0 kJ/mol. When 1.329 g of this compound (molar mass = 166.62 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter, including its contents, rose by 7.549 "C. What is the heat capacity (calorimeter constant) of the calorimeter? calorimeter constant: kJ/ "C

1. Methanol CH3OH is a potential source of fuel. An experiment was conducted to determine the enthalpy of combustion of methanol. 2.00 g of methanol was used to heat 150 g of water. The temperature of the water increased from 25°C to 87 °C. (Given that the specific heat capacity of water is 4.18 J K-1 g-1) Define the term standard enthalpy of combustion with reference to methanol. Use the data above to determine the enthalpy of combustion of methanol (show solutions).   2. Calculate the e.m.f of the following cell in the image (show solutions).

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

The heat of combustion of ethanol, C2HOH(1), is-1367 kJ/mol. A batch of sauvignon blanc wine contains 12.1 % ethanol by mass. Part A You may want to reference (Pages 191 - 192) Section 5.8 while completing this problem. Assuming the density of the wine to be 1.0 g/mL, what is the caloric content due to the alcohol (ethanol) in a 6-oz glass of wine (177 mL)? Express your answer using two significant figures. ΑΣΦ Cal Submit Request Answer < Return to Assignment Provide Feedback Esc DII F1 F2 F3 F4 PrtScn Home End F5 F6 F7 F8 F9 F10 II