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0.5060 grams of liquid cyclohexanol (C6H11OH) undergo complete combustion in a bomb calorimeter. The calorimeter assembly has a heat capacity of 827.0 J/° C and contains exactly 1000 grams of water. What is the final temperature if the initial water temperature is 24.98 ° C? The heat of combustion of the cyclohexanol is –3727 kJ/mol.

Which of the following equations would NOT be used to determine the ΔHrxn of CH₄ (g) + NH₃ (g) → HCN (g) + 3 H₂ (g) using Hess’ Law. a. N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)  b. C(s) + 2 H₂ (g) → CH₄ (g)                   c. H₂ (g) + 2 C(s) + N₂ (g) → 2 HCN (g)  d. H₂ (g) + 1/2 O₂ (g) → H₂O (l)

Calculate the heat evolved in the reaction (q). (absolute value, no units) 

Calculate the ∆H (kJ) of the reaction per mole of lead (II) nitrate consumed (here you must use a negative sign if the process is exothermic). 

What is the best reason for why either Kelvins or degrees Celsius could be used in calorimetry problems.

Which +2 ion has the same configuration?

What is the maximum number of electrons that can have the following set of quantum numbers? n = 4, ℓ = 3, mℓ = 3, ms = -½

Which of these statements is true concerning the following reaction? Na(g) → Na⁺(g) + e⁻.

If a piece of cadmium (c = .232 J/g°C) with a mass of 37.6 g and a temperature of 100.°C is dropped into 25 g of water at 23°C, what will the final temperature of the system be in °C? 

A 0.50 gram sample of NH4NO3 is added to 35.0 grams of water in a “coffee cup” (constant pressure) calorimeter and stirred until it dissolves. The temperature of the solution drops from 22.7 °C to 21.6°C. What is the HEAT OF SOLUTION of NH4NO3 expressed in kJ/mol NH4NO3?