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Dmitrij [34]
4 years ago
14

If the relative errors of three quantities to be multiplied together are 0.009, 0.006 and 0.003, what is the relative error of t

he resulting quantity? Give your answer to three decimal places
Chemistry
1 answer:
Dima020 [189]4 years ago
4 0

Answer: The relative error of the resulting quantity is 0.018.

Explanation: Relative error of the quantities when are multiplied together is usually less than or equal to the sum of each relative error. Mathematically, it is represented as

\delta x=\frac{\Delta x}{x}

According to the question,

Let us assume that the three quantities are r_1,r_2\text{ and }r_3

r=r_1\times r_2\times r_3

Taking log on both the sides, we get

log(r)=log(r_1\times r_2\times r_3)

log(r)=log(r_1)+log(r_2)+log(r_3)

Relative error is calculated by:

\frac{\delta r}{r}=\frac{\delta r_1}{r_1}+\frac{\delta r_2}{r_2}+\frac{\delta r_3}{r_3}

\frac{\delta r}{r}=0.009+0.006+0.003=0.018

This value has 3 significant figures only, so the resulting relative error is 0.018.

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if Fe(NO3)3 is dissolved in enough water to make exactly 323 ml of solution, what is the molar concentartion of nitrate ion g
Ilya [14]

The given question is incomplete. the complete question is : If 5.15 gFe(NO_3)_3 is dissolved in enough water to make exactly 323 ml of solution, what is the molar concentartion of nitrate ion.

Answer:  The molar concentartion of nitrate ion is 0.195.

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

Given : 5.15 g of Fe(NO_3)_3 is dissolved

Volume of solution = 323 ml

Molarity=\frac{n\times 1000}{V_s}

where,

n= moles of solute

Moles=\frac{\text{Given mass}}{\text{Molar mass}}=\frac{5.15g}{242g/mol}=0.021moles  

V_s = volume of solution = 323 ml

Molarity=\frac{0.021\times 1000}{323}=0.065M

As 1 M of Fe(NO_3)_3 gives 3 M of NO_3^- ions.

Thus 0.065 M of Fe(NO_3)_3 gives  = \frac{3}{1}\times 0.065=0.195M of NO_3^- ions.

The molar concentartion of nitrate ion is 0.195.

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3 years ago
How many protons and electrons are present in a Ca2+ ion?
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Considering the following precipitation reaction: Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) Which ion would NOT be present in
Allisa [31]

Answer:

The question is incomplete and confusing.

  • In the complete ionic equation you write all the ions that are formed. Those are: Pb²⁺, NO₃⁻, K⁺, and I⁻. They all are present in the complete ionic equation.

  • In the net ionic equation, the spectator ions do not appear. They are: NO₃⁻ and K⁺. They would not be present in the net ionic equation, but they do in the complete ionic equation.

See below the details.

Explanation:

Which compound will not form ions?

<u />

<u>1. Write the balanced molecular equation:</u>

  • Pb(NO₃)₂(aq) + 2KI(aq) → PbI₂(s) + 2KNO₃(aq)

<u />

<u>2. Write the ionizations for the ionic aqueous compounds:</u>

<u />

  • Pb(NO₃)₂(aq) →  Pb⁺²(aq) + 2NO₃⁻(aq)

  • 2KI(aq) → 2K⁺(aq) + 2I⁻(aq)

  • 2KNO₃(aq) → 2K⁺(aq) + 2NO₃⁻(aq)

<u />

<u>3. Write the complete ionic equation:</u>

Pb⁺²(aq) + 2NO₃⁻(aq) + 2K⁺(aq) + 2I⁻(aq) → PbI₂(s) +  2K⁺(aq) + 2NO₃⁻(aq)

Hence, since PbI₂(s) does not ionize, but stays in solid form, it will not form ions.

All, Pb⁺², NO₃⁻, K⁺, and I⁻ will be present in the total ionic equation.

It is in the net ionic equation that the spectator ions are removed. Those, are NO₃⁻ and K⁺, because they are on both sides of the complete ionic equation.

3 0
3 years ago
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