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3 years ago

An atom is made of 16 protons, 17 neutrons, and 18 electrons. What is the mass number of

Chemistry

1 answer:

Nataliya [291]3 years ago

6 0

Answer:

The answer is 33 .

Explanation:

The mass number of an atom is the atomic mass which consists of proton and neutron. This atom has 16 protons and 17 neutrons so it has a mass of 33 :

proton number + neutron number = nucleon number / atomic mass

16 + 17 = 33

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The molar solubility of zns is 1.6 Ã 10-12 m in pure water. Calculate the ksp for zns.

Oksi-84 [34.3K]

Answer:

The solubility product of zinc sulfide is $2.56\times 10^{-24}$ .

Explanation:

Solubility of the zinc sulfide = $S=1.6\times 10^{-12}$

$ZnS\rightleftharpoons Zn^{2+}+S^{2-}$

S S

The expression of solubility product is given by :

$K_{sp}=[Zn^{2+}]\times [S^{2-}]$

$K_{sp}=S\times S=S^2$

$=1.6\times 10^{-12}\times 1.6\times 10^{-12}=2.56\times 10^{-24}$

The solubility product of zinc sulfide is $2.56\times 10^{-24}$ .

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3 years ago

Arman is working on his homework four statements from his homework or below use yes or no to indicate whether each statement is

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3 years ago

Perform the calculations and determine the absolute and percent relative uncertainty. Express each answer with the correct numbe

Lana71 [14]

Answer:

Explanation:

Given the equation:

$\implies \dfrac{[9.8(\pm0.3)-2.31(\pm 0.01)]}{8.5(\pm0.6)}$

The absolute uncertainty in a measurement is the term used to describe the degree of inaccuracy.

The first step is to determine the algebraic value on the numerator.

Algebraic value = 9.8 - 231

= 7.49

The absolute uncertainty = $\sqrt{(abs. uncertainty_{v_1})^2+(abs. uncertainty_{v_2})^2}$

absolute uncertainty = $\sqrt{(0.3)^3 + (0.01)^2}$

= $\sqrt{0.09 + 0.0001}$

= 0.300167

∴

[9.8(±0.3) - 2.31(±0.01)] = 7.49(±0.300167)

The division process now is:

$\implies \dfrac{[9.8(\pm0.3)-2.31(\pm 0.01)]}{8.5(\pm0.6)}= \dfrac{7.49 (\pm 0.300167)}{8.5 (\pm0.6)}$

Relative uncertainty = $\dfrac{(\pm 0.300167)}{7.49}\times 100 \ , \ \dfrac{(\pm 0.6) }{8.5} \times 100$

Relative uncertainty = ±4.007565% , ±7.058824%

$\text{Relative uncertainty} = \sqrt{(4.007565)^2+(7.058824)^2}$

$\text{Relative uncertainty} = \sqrt{16.06057723+49.82699626}$

$\text{Relative uncertainty} = \sqrt{65.88757349}$

$\text{Relative uncertainty} = 8.117116$

≅ 8%

The algebraic value = $\dfrac{7.49}{8.5}$

= 0.881176

≅ 0.88

The percentage of the relative uncertainty = $\dfrac{\text{Absolute uncertainty }}{\text{calculated value} }\times 100$

By cross multiplying:

$\text{Absolute uncertainty} (\%) = \dfrac{\text{relative uncertainty} \times \text{calculated value}}{100}$

$\text{Absolute uncertainty} (\%) = \dfrac{8.117116\times 0.881176}{100}$

$\text{Absolute uncertainty} (\%) = 0.0715260$

$\mathbf{\text{Absolute uncertainty} (\%) \simeq 0.07}$

Finally:

$\mathbf{\implies \dfrac{[9.8(\pm0.3)-2.31(\pm 0.01)]}{8.5(\pm0.6)}= 0.88 \pm (0.07) \pm 8\%}$

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3 years ago