The volume of 0. 250 mole sample of
gas occupy if it had a pressure of 1. 70 atm and a temperature of 35 °C is 3.71 L.
Calculation,
According to ideal gas equation which is known as ideal gas law,
PV =n RT
- P is the pressure of the hydrogen gas = 1.7 atm
- Vis the volume of the hydrogen gas = ?
- n is the number of the hydrogen gas = 0.25 mole
- R is the universal gas constant = 0.082 atm L/mole K
- T is the temperature of the sample = 35°C = 35 + 273 = 308 K
By putting all the values of the given data like pressure temperature universal gas constant and number of moles in equation (i) we get ,
1.7 atm×V = 0.25 mole ×0.082 × 208 K
V = 0.25 mole ×0.082atm L /mole K × 308 K /1.7 atm
V = 3.71 L
So, volume of the sample of the hydrogen gas occupy is 3.71 L.
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The reason why the number I calculated for Avogadro’s number may match the actual number is because the comparison of the number of molecules in the top layer to the number of moles in the top layer is the definition of Avogadro’s number. It is the amount of molecules in a mole <span>of any given substance.</span>
The number of dots, electrons, surrounding the element in a Lewis diagram varies depending on what element it is, and what element it is bonding with to create a bond or several bonds. Its all dependent on what element you're being asked to make a Lewis diagram for and which elements your are boning.
Answer:
The correct answer is "0.0179".
Explanation:
The given reaction is:
⇒ ![CO_2(g) + C(s) \rightleftharpoons 2 \ CO(g)](https://tex.z-dn.net/?f=CO_2%28g%29%20%2B%20C%28s%29%20%5Crightleftharpoons%20%202%20%5C%20CO%28g%29)
The given value is:
At 727°C temperature,
Kp = 1.47
As we know,
Gas constant,
R = 0.0821 L atm/mol.K
Temperature,
= ![727+273](https://tex.z-dn.net/?f=727%2B273)
= ![1000 \ K](https://tex.z-dn.net/?f=1000%20%5C%20K)
Now,
The change in moles will be:
⇒ ![\Delta n=Products-reactants](https://tex.z-dn.net/?f=%5CDelta%20n%3DProducts-reactants)
⇒ ![=2-1](https://tex.z-dn.net/?f=%3D2-1)
⇒ ![=1](https://tex.z-dn.net/?f=%3D1)
As we know,
⇒ ![K_p=K_c(RT)^{\Delta n}](https://tex.z-dn.net/?f=K_p%3DK_c%28RT%29%5E%7B%5CDelta%20n%7D)
On substituting the given values, we get
⇒ ![1.47=K_c(0.0821\times 1000)^1](https://tex.z-dn.net/?f=1.47%3DK_c%280.0821%5Ctimes%201000%29%5E1)
⇒ ![K_c=\frac{1.47}{0.0821\times 1000}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B1.47%7D%7B0.0821%5Ctimes%201000%7D)
⇒ ![=\frac{1.47}{82.1}](https://tex.z-dn.net/?f=%3D%5Cfrac%7B1.47%7D%7B82.1%7D)
⇒ ![=0.0179](https://tex.z-dn.net/?f=%3D0.0179)