At 35.0°C and 3.00 atm pressure, a gas has a volume of 1.40 L. What pressure does the gas have at 0.00°C and a volume of 0.950 L
2 answers:
Answer:
The final pressure is 3.92 atm
Explanation:
<u>Given:</u>
<em>Initial conditions </em>
Temperature, T1 = 35.0 C
Pressure, P1 = 3.00 atm
Volume, V1 = 1.40 L
<em>Final conditions</em>
Temperature, T2 = 0.0 C
Volume, V2 = 0.950 L
<u>To determine:</u>
Final pressure, P2
<u>Explanation:</u>
Based on the ideal gas equation
where P = pressure, V = volume ; n = moles of gas
R = gas constant, T = temperature
At constant n, the above equation becomes:
Therefore,
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Answer: 2.88×atoms
Explanation: First, using stoichiometry, we must convert this from grams to moles, then from moles to atoms.
1. For the first step, we should also look at the periodic table to find the molar mass of the compound, then use that as the denominator.
2. Now that it is converted to moles, we must convert it to atoms by multiplying it by Avogadro's number.
With this information, we know that there are total atoms in 0.680 grams
.
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