Question

On a hot summer day, the density of air at atmospheric pressure at 34.5°C is 1.1242...

On a hot summer day, the density of air at atmospheric pressure at 34.5°C is 1.1242 kg/m3.

(a) What is the number of moles contained in 1.00 m3 of an ideal gas at this temperature and pressure? mol

(b) Avogadro's number of air molecules has a mass of 2.82 ✕ 10−2 kg. What is the mass of 1.00 m3 of air? (Assume air is an ideal gas.) kg

(c) Does the value calculated in part (b) agree with the stated density of air at this temperature? (Consider that it does if the values are within 10% of each other.) Yes or no?

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
On a warm summer day, a large mass of air (atmospheric pressure 1.01×105Pa) is heated by...
On a warm summer day, a large mass of air (atmospheric pressure 1.01×105Pa) is heated by the ground to a temperature of 26.0 ∘C and then begins to rise through the cooler surrounding air. 1.Calculate the temperature of the air mass when it has risen to a level at which atmospheric pressure is only 8.60×104 Pa . Assume that air is an ideal gas, with γ=1.40. (This rate of cooling for dry, rising air, corresponding to roughly 1 ∘C per...
The density of uncompressed air is 1.293 kg/m3, and one mole of air (containing Avogadro's number...
The density of uncompressed air is 1.293 kg/m3, and one mole of air (containing Avogadro's number of molecules) has a mass of 28.94 g. a) Use the density and the volume of the uncompressed air 45 cc to determine the mass of the air in the syringe, mair, in grams. (You will have to do some unit conversions.) mair =  ______ g b)Use the mass of one mole of air and Avogadro's number to determine N, the number of molecules in...
If the molecular weight of air is 28.9, what is the density of air at atmospheric...
If the molecular weight of air is 28.9, what is the density of air at atmospheric pressure and a temperature of 368.7 K? 1 atm = 1.013×105 N/m2, the mass of a proton is 1.67262 × 10?27 kg , Avogadro’s number is 6.02214 × 1023 mol?1 and k = 1.38065 × 10?23 N · m/K . Answer in units of kg/m3.
Air (a diatomic ideal gas) at 26.5°C and atmospheric pressure is drawn into a bicycle pump...
Air (a diatomic ideal gas) at 26.5°C and atmospheric pressure is drawn into a bicycle pump (see figure below) that has a cylinder with an inner diameter of 2.50 cm and length 47.0 cm. The downstroke adiabatically compresses the air, which reaches a gauge pressure of 8.00 105 Pa before entering the tire. We wish to investigate the temperature increase of the pump. The pump is made of steel that is 1.80 mm thick. Assume 4.00 cm of the cylinder's...
1.How many air molecules are in a 14.5×12.0×10.0 ft room? Assume atmospheric pressure of 1.00 atm,...
1.How many air molecules are in a 14.5×12.0×10.0 ft room? Assume atmospheric pressure of 1.00 atm, a room temperature of 20.0 ∘C, and ideal behavior. Volume conversion:There are 28.2 liters in one cubic foot. 2. At an underwater depth of 255 ft , the pressure is 8.33 atm What should the mole percent of oxygen be in the diving gas for the partial pressure of oxygen in the mixture to be 0.21 atm, the same as in air at 1...
How many air molecules are in a 15.0×12.0×10.0 ft room? Assume atmospheric pressure of 1.00 atm,...
How many air molecules are in a 15.0×12.0×10.0 ft room? Assume atmospheric pressure of 1.00 atm, a room temperature of 20.0 ∘C, and ideal behavior. Volume conversion:There are 28.2 liters in one cubic foot.
Calculate the temperature and the density of atmospheric air at 3600 m altitude, when the field...
Calculate the temperature and the density of atmospheric air at 3600 m altitude, when the field of atmospheric pressures is given by the expression: p = p0 (1 - cz) ^(5.25) where z is the altitude,and p0 and c are constants p0 = 0.1x10^6Pa c = 0.021km^(-1). Consider the air as an ideal gas of molar mass M = 0.029kg/mol
Air with a mass of 2 kg is heated at a constant pressure of 200 kPa...
Air with a mass of 2 kg is heated at a constant pressure of 200 kPa to a temperature of 500°C. Calculate the entropy change if the initial volume is 0.8 m3. Take ???? = 1.00 kJ/kg ? K and model air as an ideal gas. (Hint: Use the appropriate TdS [Gibbs] relation to calculate entropy change.)
The air in a hot-air balloon at 786 torr is heated from 19.0°C to 33.0°C. Assuming...
The air in a hot-air balloon at 786 torr is heated from 19.0°C to 33.0°C. Assuming that the moles of air and the pressure remain constant, what is the density of the air at each temperature? (The average molar mass of air is 29.0 g/mol.) Density at 19.0°C = Density at 33.0°C=
1) A hot air balloon consists of a very large bag filled with heated air at...
1) A hot air balloon consists of a very large bag filled with heated air at 120.0 °C produced from a propane burner. It has a basket hanging under it in which several people can ride. The average hot air balloon has a volume of 2.80 × 103 m3 when fully inflated. a) Determine the work (in kJ) needed to inflate the balloon under an external air pressure of 1.00 atm. b) The specific heat of the air found in...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT