I don't think so!!
Besides the fact that you're amazed at how cool the moon is.
Let suppose the Gas is acting Ideally, Then According to Ideal Gas Equation,
P V = n R T
Solving for P,
P = n R T / V ----- (1)
Data Given;
Moles = n = 1.20 mol
Volume = V = 4 L
Temperature = T = 30 + 273 = 303 K
Gas Constant = R = 0.08206 atm.L.mol⁻¹.K⁻¹
Putting Values in Eq.1,
P = (1.20 mol × 0.08206 atm.L.mol⁻¹.K⁻¹ × 303 K) ÷ 4 L
P = 7.45 atm
Answer:
91.5 mol
Explanation:
Volume of gas = 70 L
Temperature = 25°C
Pressure = 32 atm
Moles of gas = ?
Solution:
The given problem will be solve by using general gas equation,
PV = nRT
P= Pressure
V = volume
n = number of moles
R = general gas constant = 0.0821 atm.L/ mol.K
T = temperature in kelvin
Now we will convert the temperature.
25+273.15 = 298.15 K
By putting values,
32 atm × 70 L = n ×0.0821 atm.L /mol.K × 298.15 K
2240 atm.L = n ×24.48 atm.L /mol
n = 2240 atm.L / 24.48 atm.L /mol
n = 91.5 mol
Taking the average of more measurements decreases random error of measurement
Taking the average of many measurements is the most effective way to reduce random errors in a measurement. Because the certainty of the results grows as the number of data does, Less risk of random errors means that the value is more certain. Fewer measurements lead to less reliable data collection, which raises the likelihood of random errors.
The complete question is
Which procedure(s) decrease(s) the random error of a measurement: (1) taking the average of more measurements: (2) calibrating the instrument; (3) taking fewer measurements? Explain
To learn more about random errors:
brainly.com/question/14149934
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