The specific heat of air is 1.007Jg×oC and the specific heat of nitrogen (N2) is 1.040Jg×oC. What is the specific heat of oxygen (O2)?
The specific heat of air is 1.007Jg×oC and the specific heat of nitrogen (N2) is 1.040Jg×oC....
A) Compute the specific heat capacity at constant volume of nitrogen (N2) gas. The molar mass of N2 is 28.0 g/mol. the answer is: 741 J/(kg*k) B) You warm 1.55kg of water at a constant volume from 23.0?C to 29.0?C in a kettle. For the same amount of heat, how many kilograms of 23.0?C air would you be able to warm to 29.0?C? Make the simplifying assumption that air is 100% N2. C) What volume would this air occupy at...
The air that we breathe is composed of 78% nitrogen (N2), 21% oxygen (O2), and the other 1% includes water vapor, carbon dioxide, and pollutants. If a tire is inflated to a pressure of 33 pounds per square inch (psi) with regular air, what is the partial pressure of nitrogen and of oxygen within the tire?
the reaction between oxygen and nitrogen gases at high temperatures contribute to air pollution: N2(g) + O2 = 2 NO ; Kc 1.0*10^-5 at 1500 K ; suppose air has [N2] = 0.080 M and [O2] =0.020 M what is the concentration of NO at equilibrium (do it using small x approximation and don't use quadratic formula)
We can determine the molecular mass of air by considering nitrogen (N2), oxygen (O2) and argon (Ar) make up 78%, 21% and 1% of the atmosphere. The atomic masses of nitrogen, oxygen and argon are 14, 16, 40 grams/mole. Compute the molecular mass of air.
15.0 g of liquid nitrogen (N2 (l)) at 77K and a specific heat of 2.04 J/gC is added to a coffee cup calorimeter filled with 115 g of water (specific heat = 4.184 J/gC) at 37C, what is the final temperature of the water? Note: this question ignores the phase change that liquid nitrogen undergoes for simplicity at this point in the course.
A. Based on this question: The reaction between nitrogen and oxygen is given below: N2(g) + O2(g) +2 NO(g) We therefore know that which of the following reactions can also occur? Check which reaction below can occur based on the reaction between nitrogen and oxygen given at N2(g) + O2(g) +2 NO(g) 2 NO(g) + O2(g) 2 NO2(g) 2 NO(g) N2(g) + O2(g) 2 NO2(g) 2 NO(g) + O2(g) or none of the above B. Based on this question: The...
Air a. What is the volume of air in the room where you are right now? (You can measure the length, width, and height of the room with a measuring tape, or you can estimate these quantities. Just make sure you convert your answer to SI units.) b. What is the temperature in this room? (in SI units) c. Look up the current barometric pressure in your area, and convert it to SI units. d. Use the information from steps...
Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g) + O2(g) <--> 2NO(g) The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a 2.00 L container is charged with 5.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, (i) what will be the equilibrium partial pressure of nitrogen, PN2, and (ii) how many grams of O2(g) are present at equilibrium?...
When nitrogen gas is combined with oxygen gas to form nitrogen monoxide, according to the reaction N2 + O2 → 2NO, what can be used to measure the rate of the reaction? Group of answer choices: A) N2 consumption B) NO formation C) Both A and B D) O2 production
A rigid container holds both oxygen gas (O2) and nitrogen gas (N2) at 100°C. The atomic mass numbers for nitrogen and oxygen atoms are 14 and 16 respectively. Which statement describes their rms speeds? A. Vrms of O2 < Vrms of N2 B. Vrms of O2 = Vrms of N2 C. Vrms of O2 > Vrms of N2 D. All of the above. E. None of the above.