At what temperature would 0.500 moles of gas particles stored in a 100.0 mL container reach a pressure of 15.0 atm?
2 answers:
Answer: Option (C) is the correct answer.
Explanation:
According to ideal gas law, product of pressure and volume equals n times R times T.
Mathematically, PV = nRT
where P = pressure
V = volume
n = number of moles
R = gas constant
T = temperature
Since it is known that value R = 0.082 L and the other values are given as P = 15.0 atm, V = 100 mL = 0.1 L, and n = 0.5 moles.
Therefore, calculate value of temperature as follows.
PV = nRT
=
T = 36.58 K
Thus, we can conclude that temperature is 36.5 K.
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Answer:
Approximately 1.9 kilograms of this rock.
Explanation:
Relative atomic mass data from a modern periodic table:
- Pb: 207.2;
- S: 32.06.
To answer this question, start by finding the mass of Pb in each kilogram of this rock.
89% of the rock is . There will be 890 grams of
in one kilogram of this rock.
Formula mass of :
.
How many moles of formula units in that 890 grams of
?
.
There's one mole of in each mole of
. There are thus
of
in one kilogram of this rock.
What will be the mass of that of
?
.
In other words, the in 1 kilogram of this rock contains
of lead
.
How many kilograms of the rock will contain enough to provide 1.5 kilogram of
?
.
We shall consider V, the volume and T, the temperature.
According to Boyle's Laws:
In our case:
According to Boyle's Laws:
In our case: