The total pressure of a mixture of gases can be defined as the sum of the pressures of each individual gas: Ptotal=P1+P2+…+Pn. + P n . The partial pressure of an individual gas is equal to the total pressure multiplied by the mole fraction of that gas.
<u>We are given:</u>
P1 = 3 atm T1 = 623 K <em>(350 + 273)</em>
P2 = x atm T2 = 523 K <em>(250 + 273)</em>
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<u>Solving for x:</u>
From the idea gas equation:
PV = nRT
since number of moles (n) , Volume (V) and the Universal Gas constant(R) are constants;
P / T = k (where k is a constant)
the value of k will be the same for a gas with variable pressure and temperature and constant moles and volume
Hence, we can say that:
P1 / T1 = P2 / T2
3 / 623 = x / 523
x = 523 * 3 / 623
x = 2.5 atm (approx)
Therefore, the final pressure is 2.5 atm
If it is heated while it is being compressed or held inside a container as such, the pressure build up while in the container and the pressure can become so much that the container will burst.
Answer:
will be 90054 J
Explanation:
Number of moles = (mass)/(molar mass)
Molar mass of 
= 134.45 g/mol
So, 1.00 g of = 
of = 0.00744 mol of
0.00744 mol of produces 670 J of heat
So, 1 mol of produces 
of heat or 90054 J of heat
Answer:
λ = 0.45×10⁻⁶ m
Explanation:
Given data:
Wavelength of blue light = ?
Frequency of blue light = 6.69×10¹⁴ s⁻¹
Solution:
Formula;
Speed of wave = wavelength × frequency
Speed of wave = 3.00×10⁸ m/s
by putting vales,
3.00×10⁸ m/s = λ × 6.69×10¹⁴ s⁻¹
λ = 3.00×10⁸ m/s / 6.69×10¹⁴ s⁻¹
λ = 0.45×10⁻⁶ m
