A 6.55 g sample of aniline (C6H5NH₂, M = 93.13 g/mol) was combusted in a bomb calorimeter. If the temperature rose by 32.9°C, use the information below to determine the heat capacity of the calorimeter. 4C6H5NH₂(I) + 350₂(g) → 24CO₂(g) + 14H₂O(g) + 4NO₂(g) A,H° -1.28 x 104 kJ/mol

A 6.55 g sample of aniline (C6H5NH₂, M = 93.13 g/mol) was combusted in a bomb calorimeter. If the temperature rose by 32.9°C, use the information below to determine the heat capacity of the calorimeter. 4C6H5NH₂(I) + 350₂(g) → 24CO₂(g) + 14H₂O(g) + 4NO₂(g) A,H° -1.28 x 104 kJ/mol

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

Similar questions

Consider the thermochemical equation for the combustion of acetone (C3H₂O), the main ingredient in nail polish remover: C3H6O (1) + 4 O₂ (g) → 3 CO₂ (g) + 3 H₂O (g) ΔΗ° rxn = 1790 kJ If a bottle of nail polish remover contains 222 mL of acetone, what is the magnitude (the value) of heat released by the complete combustion of the acetone in the bottle? The density of acetone is 0.788 g/mL. The molar mass of acetone is 58.08 g/mol. The units are kJ. Do not include units in your answer.
A researcher studying the nutritional value of a new candy places a 5.60 g5.60 g sample of the candy inside a bomb calorimeter and combusts it in excess oxygen. The observed temperature increase is 2.41 ∘C.2.41 ∘C. If the heat capacity of the calorimeter is 47.50 kJ⋅K−1,47.50 kJ⋅K−1, how many nutritional Calories are there per gram of the candy?
What is the heat capacity (Cp) of a 7.5 g piece of tin if its temperature changes by 12.3°C when it is supplied with 20 J from a Bunsen burner?
A 57.0g sample of aluminum is put into a calorimeter (see sketch at right) that contains 250.0g of water. The aluminum sample starts off at 96.9°C and the temperature of the water starts off at 23.0°C. When the temperature of the water stops changing it's 26.2°C. The pressure remains constant at 1atm. Calculate the specific heat capacity of aluminum according to this experiment. Be sure your answer is rounded to 2 significant digits. Please type answer note write by hend.
A piece of metal of mass 15 g at 99◦C is placed in a calorimeter containing 41.3 g of water at 19◦C. The final temperature of the mixture is 40.2◦C. What is the specific heat capacity of the metal? Assume that there is no energy lost to the surroundings. Answer in units ofJg·◦C.
A 2.30 g sample of ethanol, CH3CH2OH, is combusted in a bomb calorimeter. The temperature of the calorimeter increases by 4.89 K. If the heat capacity of the bomb is 663 J/K and it contains 2.57 kg of water, what is the enthalpy change per mole of ethanol combusted? The specific heat capacity of water is 4.18 J/g×K and the molar mass of ethanol is 46.07 g/mol.
A researcher studying the nutritional value of a new candy places a 6.00 g6.00 g sample of the candy inside a bomb calorimeter and combusts it in excess oxygen. The observed temperature increase is 2.89 ∘C.2.89 ∘C. If the heat capacity of the calorimeter is 45.80 kJ⋅K−1,45.80 kJ⋅K−1, how many nutritional Calories are there per gram of the candy?
Calculate the energy required to heat 0.30kg of graphite from −4.8°C to 13.1°C . Assume the specific heat capacity of graphite under these conditions is 0.710J·g−1K−1 . Be sure your answer has the correct number of significant digits.
The molar heat capacity of silver is 25.35 J/mol⋅∘C . How much energy would it take to raise the temperature of 8.60 g of silver by 14.4 ∘C?
5.00 × 10−2 mol KOH and an excess of hydrochloric acid are combined in 100.0 mL of water initially at 25.0 °C, leading to a final measured temperature of 31.1 °C. (a) What is the heat flow for the water in the calorimeter, qH2O, in Joules? (b) Assuming the calorimeter constant Ccal = 50.0 J °C , what is the heat flow for the calorimeter, qcal, in Joules? (c) What is the amount of heat given off by the reaction, qrxn, in Joules? (d) What is the molar enthalpy of the neutralization reaction (shown below) as measured in the calorimeter, ∆H◦ rxn in kilojoules per mole? H3O + (aq) + OH– (aq) → 2H2O (l)
A chemist carefully measures the amount of heat needed to raise the temperature of a 531.0mg sample of C9H10O2 from 40.1°C to 58.2°C . The experiment shows that 15.1J of heat are needed. What can the chemist report for the molar heat capacity of C9H10O2 ? Be sure your answer has the correct number of significant digits. ⋅J⋅mol−1K−1
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 0.3215 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.162×10 g of water. During the combustion the temperature increases from 25.15 to 27.48 °C. The heat capacity of water is 4.184 J glc-!. The heat capacity of the calorimeter was determined in a previous experiment to be 769.3 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phenanthrene based on these data. C14H10(s) + (33/2) O,(g) – → 5 H,O(1) + 14 CO2(g) + Energy Molar Heat of Combustion = kJ/mol