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The correct answer is B. Electrons will be added to an atom starting from the lowest possible level or sublevel.
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The question mentions a change in temperature from 25 to 50 °C. With that, the aim of the question is to determine the change in volume based on that change in temperature. Therefore this question is based on Gay- Lussac's Gas Law which notes that an increase in temperature, causes an increase in pressure since the two are directly proportional (once volume remains constant). Thus Gay-Lussac's Equation can be used to solve for the answer.
Boyle's Equation:

=

Since the initial temperature (T₁) is 25 C, the final temperature is 50 C (T₂) and the initial pressure (P₁) is 103 kPa, then we can substitute these into the equation to find the final pressure (P₂).

=

∴ by substituting the known values, ⇒ (103 kPa) ÷ (25 °C) = (P₂) ÷ (50 °C)
⇒ P₂ = (4.12 kPa · °C) (50 °C)
=
206 kPa
Thus the pressure of the gas since the temperature was raised from 25 °C to 50 °C is
206 kPa
Answer:
134K
Explanation:
Using the ideal gas law equation;
PV = nRT
Where;
P = pressure (atm)
V = volume (Litres)
n = number of moles (mol)
R = gas constant (0.0821 Latm/Kmol)
T = temperature (K)
Based on the information provided, n = 1.4moles, P = 3.25atm, V = 4.738L, T = ?
3.25 × 4.738 = 1.4 × 0.0821 × T
15.3985 = 0.11494T
T = 15.3985/0.11494
T = 133.969
Approximately;
T = 134K
Answer:
1.38×10^25 molecules
Explanation:
Applying n= (no. of molcules)/NA
23 = N/6.02×10^23
= 1.38×10^25 molecules
Answer:
Volume of the gass will decrease by three times of the original volume
Explanation:
Volume is inversly propotional to the pressure applied on it.