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Angelina_Jolie [31]
3 years ago
5

Explain the differences between an ideal gas and a real gas.

Chemistry
1 answer:
Annette [7]3 years ago
3 0

Answer:

Ideal Gas

The ideal gas is extremely small and the mass is almost zero and no volume Ideal gas is also considered as a point mass.

Real Gas

The molecules of real gas occupy space though they are small particles and also have volume.

Explanation:

I think i did this right

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Will give brainliest!!
Nikolay [14]

Answer: True.

Explanation: A teakettle does have a greater frequency than a drumbeat.  The teakettle has a higher pitched sound and frequency than a low pitched sound like a drumbeat. So a teakettle is high and a drumbeat is low.

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2 years ago
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Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is th
kolbaska11 [484]

Answer: When using 645 L /s  of O2 in a temperature and pressure of  195°C,  0.88 atm  respectively, we will get 0.355Kg /s NO

Explanation:

  • First we review the equation that represents the oxidation process of the NH3 to NO.

4NH3(g) + 5O2(g) ⟶4 NO(g) +6 H2O(l)  

  • Second we gather the information what we are going to use in our calculations.

O2 Volume Rate = 645 L /s

Pressure = 0.88 atm

Temperature = 195°C + 273 = 468K

NO molecular weight = 30.01 g/mol  

  • Third, in order to calculate the amount of  NO moles produced by 645L/ s of O2, we must find out, how many moles (n) are 645L O2 by using the general gas equation PV =n RT

Let´s keep in mind that using this equation our constant R is 0.08205Lxatm/Kxmol

PV =n RT

n= PV / RT

n= [ 0.88atm x 645L/s] / [ (0.08205 Lxatm/Kxmol) x 468K]

n= 14.781 moles /s of O2

  • Fourth, now by knowing the amount of moles of O2, we can use the equation to calculate how many moles of NO will be produced and then with the molecular weight, we will finally know the total mass per second .

14.781 moles /s of O2 x 4moles NO / 5 moles O2 x  30.01g NO / 1 mol NO x 1Kg NO /1000g NO = 0.355Kg /s NO

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3 years ago
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Yakvenalex [24]
<span>a thermodynamic quantity representing the unavailability of a system's thermal energy for conversion into mechanical work, often interpreted as the degree of disorder or randomness in the system.</span>
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3 years ago
I’m putting 50 points into this I need help badly bro
KIM [24]

1. P = F/A; weight is a force (the force of gravity on an object), so divide the weight by the area given. P = 768 pounds/75.0 in² = 10.2 pounds/in².

2. Using the same equation from question 1, rearrange it to solve for A: A = F/P. We're given the force (the weight) and the pressure, so A = 125 pounds/3.25 pounds/in² = 38.5 in².

3. Again, using the same equation from question 1, rearrange it this time to solve for F: F = PA = (4.33 pounds/in²)(35.6 in²) = 154 pounds.

4. We can set up a proportion given that 14.7 PSI = 101 KPa. This ratio should hold for 23.6 PSI. In other words, 14.7/101 = 23.6/x; to solve for x, which would be your answer, we compute 23.6 PSI × 101 kPa ÷ 14.7 PSI = 162 kPa.

5. We are told that 1.00 atm = 760. mmHg, and we want to know how many atm are equal to 854 mmHg. As we did with question 4, we set up a proportion: 1/760. = x/854, and solve for x. 854 mmHg × 1.00 atm ÷ 760. mmHg = 1.12 atm.

6. The total pressure of the three gases in this container is just the sum of the partial pressures of each individual gas. Since our answer must be given in PSI, we should convert all our partial pressures that are not given in PSI into PSI for the sake of convenience. Fortunately, we only need to do that for one of the gases: oxygen, whose partial pressure is given as 324 mmHg. Given that 14.7 PSI = 760. mmHg, we can set up a proportion to find the partial pressure of oxygen gas in PSI: 14.7/760. = x/324; solving for x gives us 6.27 PSI oxygen. Now, we add up the partial pressures of all the gases: 11.2 PSI nitrogen + 6.27 PSI oxygen + 4.27 PSI carbon dioxide = 21.7 PSI, which is our total pressure.

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3 years ago
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