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3 years ago

What is the percent error when a student measures the volume to be 19.3 liters when

Chemistry

1 answer:

katrin2010 [14]3 years ago

7 0

Answer:

The answer is

Explanation:

The percentage error of a certain measurement can be found by using the formula

$P(\%) = \frac{error}{actual \: \: number} \times 100\% \\$

From the question

actual volume = 22.4 L

error = 22.4 - 19.3 = 3.1

The percentage error is

$P(\%) = \frac{3.1}{22.4} \times 100 \\ = 13.839285714...$

We have the final answer as

Hope this helps you

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What is the total pressure of a gas mixture containing partial pressures of

Advocard [28]

Answer:

1.54 atm

Explanation:

By Dalton's Law Of partial pressure,

Total Pressure = Sum of all partial pressures

So,P= P1 + P2 + P3

Therefore, P=0.23+0.42+0.89

=1.54 atm

8 0

3 years ago

Using the fact that at 0.10 M, the absorbance was 0.357; and at 0.20 M, the absorbance was 0.714, the absorptivity (slope) is

olga_2 [115]

Answer:

The answer is "3.57 and 0.07".

Explanation:

Using the slop formula:

$=\frac{n_2-n_1}{n_2-n_1}\\\\ =\frac{0.714-0.357}{0.20-0.10} \\\\ = ABSORPTIVITY, \ \ a=3.57 \\\\A= a\times b \times c$

Given:

$A=0.250$

length path $b=1$

from calibration it is found that

$a=3.57\\\\consentation \ c=\frac{A}{a\times b} \\\\C=\frac{0.250}{3.57\times 1}$

$=0.07 \ M$

3 0

3 years ago

What volume (in liters) of a solution contains 0.14 mol of KCl?

oksano4ka [1.4K]

Answer:

$\boxed {\boxed {\sf 0.078 \ L }}$

Explanation:

We are asked to find the volume of a solution given the moles of solute and molarity.

Molarity is a measure of concentration in moles per liter. It is calculated using the following formula:

$molarity= \frac{moles \ of \ solute}{liters \ of \ solution}$

We know there are 0.14 moles of potassium chloride (KCl), which is the solute. The molarity of the solution is 1.8 molar or 1.8 moles of potassium chloride per liter.

moles of solute = 0.14 mol KCl
molarity= 1.8 mol KCl/ L
liters of solution=x

Substitute these values/variables into the formula.

$1.8 \ mol \ KCl/ L = \frac { 0.14 \ mol \ KCl}{x}$

We are solving for x, so we must isolate the variable. First, cross multiply. Multiply the first numerator and second denominator, then the first denominator and second numerator.

$\frac {1.8 \ mol \ KCl/L}{1} = \frac{0.14 \ mol \ KCl}{x}$

$1.8 \ mol \ KCl/ L *x = 1*0.14 \ mol \ KCl$

$1.8 \ mol \ KCl/ L *x = 0.14 \ mol \ KCl$

Now x is being multiplied by 1.8 moles of potassium chloride per liter. The inverse operation of multiplication is division, so we divide both sides by 1.8 mol KCl/L.

$\frac {1.8 \ mol \ KCl/ L *x}{1.8 \ mol \ KCl/L} = \frac{0.14 \ mol \ KCl}{1.8 \ mol \ KCl/L}$

$x= \frac{0.14 \ mol \ KCl}{1.8 \ mol \ KCl/L}$

The units of moles of potassium chloride cancel.

$x= \frac{0.14 }{1.8 L}$

$x=0.07777777778 \ L$

The original measurements of moles and molarity have 2 significant figures, so our answer must have the same. For the number we found, that is the thousandth place. The 7 in the ten-thousandth place tells us to round the 7 up to a 8.

$x \approx 0.078 \ L$