I) AH>0 shows that reaction is an exothermic. II) Mole fraction of nitrogen (N2) in air is 0.21. III) If surrounding works on system then W is positive. IV) As temperature of a gas increases its volume decreases. V) The equation (V= an) represents an equation for the Avogadro’s law. VI) Ammonia burns in oxygen to form carbon dioxide and water.

I) AH>0 shows that reaction is an exothermic. II) Mole fraction of nitrogen (N2) in air is 0.21. III) If surrounding works on system then W is positive. IV) As temperature of a gas increases its volume decreases. V) The equation (V= an) represents an equation for the Avogadro’s law. VI) Ammonia burns in oxygen to form carbon dioxide and water.

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

What is the heat capacity of 2.00 moles of liquid water?
Please help with this question
Subject :- Chemistry
Please help out I’m so confused and struggling
In a bomb calorimeter, the energy (ΔU) of CH4 gas at 25 0C and at a constant volume was measured -0.885 kJ. What is the energy (ΔH) released by burning methane gas?
One mole of CO2 gas is heated and its temperature increases by 10 K. If the same heat is given to 2 moles of H2S gas, how much does its temperature change? (Assume that the molecular vibrations don't change the heat absorption).
Write the thermochemical equation for the following reactions that occur at constant pressure. 1.Combustion of hexane, C6H12, to carbon dioxide gas and water releases 3923.9 kJ of heat.
Here is the graph below pls answer the question. thanks The graphs in this experiment are for nitrogen gas, however, they do not have labels that identify the type of gas being represented. Would the curves for a more massive gas, such as CO2, look different? O No. The molar mass of a gas does not affect the shape of the kinetic energy distribution. O Yes, since CO2 has a larger molar mass, we'd expect the curve to shift towards left, indicating that a larger fraction of molecules have low kinetic energies. O Yes, since CO2 has a larger molar mass, we'd expect the distribution to shift towards the right, indicating a larger fraction of the molecules have high kinetic energies. Boltzmann energy distribution at 300.0 K and 500.0 K 0.0002 300.0 K 0.00015 0.0001 500.0 K 0.00005 so0 10000 15000 20000 25000 30000 35000 Kinetic energy 1/mol) Fraction per l/mol
A 0.1375g sample of solid Mg is burned in a constant volume bomb calorimeter that has a heat capacity of 3024 J/0C. The temperature increases by 1.1260C. Calculate the heat given off by the burning Mg in kJ/g Mg and kJ/mole Mg
12:27 1%L7 Methane burns with a fuel value of 55.5 kJ/g. If a 1.00-L cylinder containing pure methane gas at a pressure of 3900 psi at 298 k is completely burned, how much energy will be released? energy: What mass of CO, will form in this reaction? mass of CO,:
According to the following thermochemical equation, how much heat is produced when 3.85 g of CHL is burned in excess O2. . Fall 2 CH (8) + 2 O2 (g) CO2e+2 H,O AH +2 H2O (g) AH = 802 kJ 192KJ b. 385 kJ C. 802 kJ d. 96KJ e. Not listed 5. 0OMHCL what volume of the 12 M HCl do you need? You have a solution of 12 M HCI. f you want to dilute this to a 100. mL solu
Measurements show that the energy of a mixture of gaseous reactants increases by 388. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that-88. kl of work is done on the mixture during the reaction. th Calculate the change in enthalpy of the gas macture during the reaction. Round your anawer to 3 significant digits. O exothermic Is the reaction exothermic or endothermic O endothermic