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worty [1.4K]
3 years ago
13

Larisa pumps up a soccer ball until it has a gauge pressure of 61 kilopascals. The volume of the ball is 5.2 liters. The air tem

perature is 32°C, and the outside air is at standard pressure. How many moles of air are in the ball?
Chemistry
1 answer:
kirill115 [55]3 years ago
7 0

The total ball pressure is sum of gauge pressure and atmospheric pressure

We know that atmospheric pressure = 101.325 kPa

so the total ball pressure = 61 kPa + 101.325 kPa = 162.325 kPa

Now we will use ideal gas equation as

PV = nRT

P = pressure = 162.325 kPa

V = 5.2 L

R = gas constant = 8.314 kPa  L / mol K

T = 32 C = 273.15 + 32 = 305.15 K

n = moles = ?

Moles = PV / RT = 162.325 kPa X 5.2 / 305.15 X 8.314 = 0.332 moles

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Sunny_sXe [5.5K]

Answer:

G_calculated = 1.756

The outlier should be rejected, as G_cal > G_tab (= 1.463) at 95 % confidence.

Explanation:

The Grubb's test is used for identifying an outlier in data, which is from the same population. For this, a statistical term, G, is calculated for the suspected outlier. If the calculated value is greater than the tabulated G value then the suspected value is rejected. This term is given as,

G_calculated = | suspect value - mean| / s

Here,  suspect value is 13.8, mean is to be taken of all the data (including suspected value). s is the standard deviation of the sample data.

s is calculated from the following formula:

s = (Σ(xi - x)²/(N-1))^1/2

Here, x is the mean, which is 15.24, xi is individual value and N is the total number of data (5).

From the above formula, s is found to be

Standard Deviation, s = 0.820

Now for G value,

G_calculated = | 13.8 - 15.24| / (0.820)

G_ calculated = 1.756

The tabulated G value at 95 % confidence and N -1 (5 - 1 = 4) degree of freedom is, 1.463.

As calculated G (1.756) is greater than the tabulated G (1.463), the value 13.8 is considered an outlier at 95 % confidence.  

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How many moles of LiOH are required to prepare 1.50L of 5.4 M LiOH?
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You would need 8.1 <span>moles of LiOH</span>
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