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79 solutions

Calorimetry

Q. A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.300 M HNO3 in a coffee cup calorimeter. If both solutions were initially at 35.00°C and the temperature of the resulting solution was recorded as 37.00°C, determine the ΔH°rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH and HCl. Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2) that the density and the heat capacity of the resulting solution are the same as water.

Solved • Jul 25, 2019

Calorimetry

Q. Determine the activation energy for the forward endothermic dissolution reaction

Solved • Jul 22, 2019

Calorimetry

Q. A foundry worker places a 5.78 kg sheet of nickel at a temperature of 17°C on top of a 16.7 kg sheet of palladium at 68°C. Assuming no heat is lost to the surroundings, calculate the final temperature of two sheets of metal.

Solved • Jul 18, 2019

Calorimetry

Q. Zirconium metal has a molar heat capacity of 25.4 J/mol*K. given that q = Cm x n x ΔT, how many moles of zirconium are present if 3.12 x 10^3 J of heat is required to raise the temperature of the sample by 37.5 K?

Solved • Jul 18, 2019

Calorimetry

Q. When a 0.3385 gram sample of solid calcium (Ca) was burned in a constant-volume calorimeter (bomb calorimeter) with a measured heat capacity of 0.1845 kJ/°C , the temperature of the calorimeter increased by 29.06°C. (a) Calculate the change of heat released by the combustion of the calcium sample. (b) Determine the change of heat that would be released by the combustion of 1 mole of calcium.

Solved • Jul 18, 2019

Calorimetry

Q. The amount of heat (q) gained or lost bya substance (with mass m) as its temperature changes (ΔT) depends on its specific heat capacity (Cp) according to the following equation. q = Cp x m x ΔT The quality of industrial diamonds is determined in part by measuring the specific heat capacity, which is 0.5091 J/g*K for pure diamond. If the absorption of 26.41 J of heat by a 2.14 g diamond sample of unknown purity causes its temperature to rise from 26.08°C to 73.36°C, is the diamond sample pure? Explain your reasoning. The calculated Cp is ___ J/g*K and the value for pure diamond is 0.5091 J/g*K. These values are ___, thus the sample ___ pure.

Solved • Jul 18, 2019

Calorimetry

Q. How much energy is required to convert 15.0 g of ice at -15°C to 15.0 g of steam at 113°C? Specific heat capacity, ice: 2.108 J/g*K (at 0°C) Specific heat capacity, water: 4.1801 J/g*K (at 25°C) Specific heat capacity, steam: 2.0784 J/g*K (at 100°C) ΔHfus = 333.6 J/g (at 0°C) ΔHvap = 2.2567 kJ/g (at 100°C)

Solved • Jul 18, 2019