The reaction of hydrogen gas (H2) with oxygen gas (O2) is a COMBINATION or SYNTHESIS reaction, because multiple substances combine to form fewer substances. Here, the two gases form one substance, water (H2O):
2H2 + O2 -- > 2H2O
Answer:
1. A. True
2. A. True
3. B. False
4. A. True
5. B. False
Explanation:
1. The particles are in constant motion. The collisions of the particles with the walls of the container are the cause of the pressure exerted by the gas. A. True. The pressure of an ideal gas is higher than the one that would exert a real gas.
2. The particles are assumed to exert no forces on each other; they are assumed neither to attract nor to repel each other. A. True. The intermolecular forces are negligible.
3. The particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be about 1 mL. B. False. The volume of the gas particles is negligible.
4. The molecules in a real gas have finite volumes and do exert forces on each other, thus real gases do not conform to some of the assumptions of an ideal gas as stated by the kinetic molecular theory. A. True. We cannot apply ideal gas laws to real gases.
5. The average kinetic energy of a collection of gas particles is assumed to be inversely proportional to the Kelvin temperature of the gas. B. False. The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas.
Answer:
During exercise, heart rate can rise dramatically, from a resting rate of 60–80 beats per minute to a maximum rate of about 200 for a young adult. While you are running, blood flow is diverted toward tissues that need it most. For example, muscles in the arteries in your legs relax to allow more blood flow.
Explanation:
Would it be standard notation
Answer : The rate of formation of 
is, 
Explanation : Given,
Rate of disappearance of 
= 
The given rate of reaction is,
The expression for rate of reaction :
![\text{Rate of disappearance}=-\frac{1}{2}\frac{d[NO]}{dt}=-\frac{d[Cl_2]}{dt}](https://tex.z-dn.net/?f=%5Ctext%7BRate%20of%20disappearance%7D%3D-%5Cfrac%7B1%7D%7B2%7D%5Cfrac%7Bd%5BNO%5D%7D%7Bdt%7D%3D-%5Cfrac%7Bd%5BCl_2%5D%7D%7Bdt%7D)
![\text{Rate of formation}=\frac{1}{2}\frac{d[NOCl]}{dt}](https://tex.z-dn.net/?f=%5Ctext%7BRate%20of%20formation%7D%3D%5Cfrac%7B1%7D%7B2%7D%5Cfrac%7Bd%5BNOCl%5D%7D%7Bdt%7D)
From this we conclude that,
![\frac{1}{2}\frac{d[NOCl]}{dt}=-\frac{d[Cl_2]}{dt}](https://tex.z-dn.net/?f=%5Cfrac%7B1%7D%7B2%7D%5Cfrac%7Bd%5BNOCl%5D%7D%7Bdt%7D%3D-%5Cfrac%7Bd%5BCl_2%5D%7D%7Bdt%7D)
![\frac{d[NOCl]}{dt}=2\times \frac{d[Cl_2]}{dt}](https://tex.z-dn.net/?f=%5Cfrac%7Bd%5BNOCl%5D%7D%7Bdt%7D%3D2%5Ctimes%20%5Cfrac%7Bd%5BCl_2%5D%7D%7Bdt%7D)
Now put the value of rate of disappearance of , we get:
![\frac{d[NOCl]}{dt}=2\times (4.24\times 10^{-2}M/s)=8.48\times 10^{-2}M/s](https://tex.z-dn.net/?f=%5Cfrac%7Bd%5BNOCl%5D%7D%7Bdt%7D%3D2%5Ctimes%20%284.24%5Ctimes%2010%5E%7B-2%7DM%2Fs%29%3D8.48%5Ctimes%2010%5E%7B-2%7DM%2Fs)
Therefore, the rate of formation of is,
