Element X has two isotopes. If 72.0% of the element has an isotope mass of 84.9 atomic mass units, and 28.0% of the element has
1 answer:
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<u>Answer:</u>
<u>For 1:</u> The value of for the chemical equation is -24.636 kJ/mol
<u>For 2:</u> The value of for the chemical equation is -20.925 kJ/mol
<u>Explanation:</u>
For the given chemical equation:
- <u>For 1:</u>
To calculate the for given value of equilibrium constant, we use the relation:
.....(1)
where,
= ? kJ/mol
R = Gas constant =
T = temperature = 2000 K
= equilibrium constant in terms of partial pressure = 4.40
Putting values in above equation, we get:
Converting this into kilo joules, we use the conversion factor:
1 kJ = 1000 J
So, -24636.12 J/mol = -24.636 kJ/mol
Hence, the value of for the chemical equation is -24.636 kJ/mol
- <u>For 2:</u>
The expression of for the given chemical equation is:
We are given:
Putting values in above equation, we get:
Now, calculating the value of by using equation 1:
R = Gas constant =
T = temperature = 2000 K
= equilibrium constant in terms of partial pressure = 3.52
Putting values in equation 1, we get:
Converting this into kilo joules, we use the conversion factor:
1 kJ = 1000 J
So, -20925.68 J/mol = -20.925 kJ/mol
Hence, the value of for the chemical equation is -20.925 kJ/mol
Answer:
Volume of = 15.31 mL
Volume of = 4.69 mL
Explanation:
Given that:
the density of the mixture = 1.82 g/mL
From the density of the pure samples
The density of = 1.492 g/mL
The density of = 2.890 g/mL
The total volume of the liquid mixture = 20.0 mL
Suppose the volume of = P ml
and the volume of = Q ml
the sum of their volumes should be equal to the total volume of the mixture
----- (1)
However, we know that Density = mass/volume
∴ mass = density × volume
The equation can now be expressed as:
1.492 g/mL × P mL + 2.890 g/mL × Q mL = 1.82 g/mL × 20 mL ---- (2)
From equation (1) ;
let Q = 20 - P
The replace the value of P into equation (2)
1.492 g/mL × P mL + 2.890g/mL × (20 - P) mL = 1.82 g/mL × 20 mL
1.492 P g + 57.8g - 2.890 P g = 36.4g
1.492 P g - 2.890 P g = 36.4g - 57.8g
-1.398 P g = -21.4g
P = -21.4g/-1.398g
P = 15.31 mL
Q = 20 - P
Q = (20 - 15.31) mL
Q = 4.69 mL
∴
Volume of = 15.31 mL
Volume of = 4.69 mL