Answer:
V = 22.86 L
Explanation:
Given data:
Mass of nitrogen dioxide = 45000 mg
Pressure = 1 atm
Temperature = 273 k
Volume = ?
Solution:
First of all we will convert the mass into moles.
<em>Number of moles = mass/ molar mass</em>
Number of moles <em>= </em>45 g/ 46 g/mol
Number of moles = 1.02 mol
Now we will determine the volume at STP.
PV = nRT
V = nRT/P
V = 1.02 mol × 0.0821 atm. mol⁻¹. k⁻¹. L× 273 k / 1 atm
V = 22.86 atm. L /1 atm
V = 22.86 L
Answer:
1038.96 kPa
Explanation:
We’ll use the ideal gas law; P1V1/T1 = P2V2/T2
P1*14.8/75.5 = 101.3*16.5/70.2
P1 = (101.3 * 16.5 * 75.5) / (70.2 *14.8)
P1 = 1038.96
Answer:
Left, Left, Right, Left, Right, Right
Explanation:
Follow that order!
The first one’s 10% and energy is used for movement but i’m not sure what “processes” that would be and the last one is it’s released as heat
The conditions do you expect helium gas to deviate most from ideal behavior is at <span>100 K and 1 atm. The answer is letter A. An ideal gas has a very low pressure and very low temperature.</span>