.110. Suppose that there is 2.43 mol of nitrogen gas in an insulated, sealed 31.7-L container initially at 285 K. The specific heat of nitrogen gas is 1.04 kJ kg¯1 K-1 (note units). If a 5.44-kg block of iron at 755 K is placed in this container and it is sealed again (with no loss of nitrogen), what is the final pressure of the nitrogen gas?

.110. Suppose that there is 2.43 mol of nitrogen gas in an insulated, sealed 31.7-L container initially at 285 K. The specific heat of nitrogen gas is 1.04 kJ kg¯1 K-1 (note units). If a 5.44-kg block of iron at 755 K is placed in this container and it is sealed again (with no loss of nitrogen), what is the final pressure of the nitrogen gas?

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

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.
Propane gas (C3H6 (g)) is withdrawn from a 100.0 L cylinder at 25.0 oC and is burned at constant pressure in an excess of oxygen. The pressure in the cylinder falls from 2.25 atm to 1.05 atm. The liberated heat is then used to raise the temperature of 65.5 L of water from 25.0 oC to 56.7 oC. What % of the heat of combustion was absorbed by the water (d = 1.00 g/mL)? Specific heat capacity of water = 4.18 J/g/oC Δ Hfo(H2O(l)) = -285.8 kJ/mol, Δ Hfo(O2(g)) = 0 kJ/mol, Δ Hfo(CO2 (g)) = -393.5 kJ/mol Δ Hfo(C3H6 ) = -103.8 kJ/mol
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 0.6334 g sample of acetylsalicylic acid (C9H8O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.100×103 g of water. During the combustion the temperature increases from 22.68 to 25.23 °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 929.9 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of acetylsalicylic acid based on these data. C9H8O4(s) + 9O2(g) 4 H2O(l) + 9 CO2(g) + EnergyMolar Heat of Combustion = how many kJ/mol
Calculate the heat necessary to increase temperature of a) 100. g of water b) 2.00 mol H2O(l) from 20 ℃ to 100 ℃.
The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).
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 1.1250 g sample of β-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.200×103 g of water. During the combustion the temperature increases from 23.58 to 26.40 °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 979.8 J/°C.Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of β-D-fructose based on these data.C6H12O6(s) + 6O2(g) 6 H2O(l) + 6 CO2(g) + Energy
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 0.6421 g sample of 2-naphthylacetic acid (C12H10O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.267×103 g of water. During the combustion the temperature increases from 27.50 to 30.60 °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 843.2 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 2-naphthylacetic acid based on these data. C12H10O2(s) + (27/2) O2(g) 5 H2O(l) + 12 CO2(g) + EnergyMolar Heat of Combustion = kJ/mol
A sample of iron, which has a specific heat capacity of 0.449 J.g¹.°C¹, is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The iron sample starts off at 98.2 °C and the temperature of the water starts off at 23.0 °C. When the temperature of the water stops changing it's 27.4 °C. The pressure remains constant at 1 atm. Calculate the mass of the iron sample. Be sure your answer is rounded to 2 significant digits. 1 g x10 X 5 thermometer. insulated container water sample a calorimeter
What quantity of heat (in kJ) will be released if 0.1673 mol of NH³ are mixed with 0.200 mol of O: in the following chemical reaction? 4 NH (g) + O: (g) → 2 N₂H4 (g) + 2 H₂O (g) AH = -286 kJ/mol
Hw.77.
A sample of glass, which has a specific heat capacity of 0.670 J-gec, is put into a calorimeter (see sketch at right) that insulated container contains 250.0 g of water. The glass sample starts off at 86.1 °C and the temperature of the water starts off at 18.0 °C. When the temperature of the water stops changing it's 20.3 "C. The pressure remains constant at 1 atm. Calculate the mass of the glass sample. Be sure your answer is rounded to the correct number of significant digits. 18 D.P thermometer- X water sample a calorimeter Ar
A 0.8 mol sample of a monatomic ideal gas is heated from a temperature of 88 °C to 383 °C in a 4.2 L vessel. If the size of the vessel doesn't change over the course of this process, calcuate the maximum amount of heat absorbed or emitted by the gas sample. 0 KJ-mol 1