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4 years ago

Compound for Fe2+andO2-

Chemistry

2 answers:

Butoxors [25]4 years ago

7 0

Fe2+;

Systemic name:

Iron(II)

Common name:

Ferrous

O2-;

Oxygen - O2

Superoxide anion - O2-

anygoal [31]4 years ago

6 0

Ferrous oxide or Iron (II) oxide. Brainliest? if its correct

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Which statement correctly describes a characteristic that a scientific measuring toll should have?

Gwar [14]

Answer:

Explanation:

To be accurate, it must be able to make measurements that are close to the actual value.

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3 years ago

What is the molarity if 6664 grams of boron iodide is dissolved in 5.25 liters of water?

Virty [35]

Answer:

3.24 mol/L

Explanation:

Given that:

mass of Boron triiodide = 6664 grams

molar mass of BI_3 = 391.52 g/mol

Recall that:

number of moles = mass/molar mass

∴

number of moles = 6664 g /391.52 g/mol

number of moles = 17.02 mol

Also;

Molarity = moles for solute/liter for solution

= 17.02 mol/5.25 L

= 3.24 mol/L

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3 years ago

All of the halogens have the same molecular formula. Which molecule will have the longest bond length

cluponka [151]

Answer:

Iodine (I2) has the longest bond length because the radius of the I atom is greater that the radii of the other halogen atoms.

Explanation:

here

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2 years ago

It takes 2,267 joules of heat to raise the temperature of a 44.5 gram sample of a metal from 33.9°C to 288.3°C. What is the heat

ehidna [41]

Answer:

$\boxed{\text{0.200 J$^{\circ}$C$^{-1}$g$^{-1}$}}}$

Explanation:

The formula for the amount heat q absorbed by a substance is

q = mcΔT

where

m = the mass of the substance

C = the specific heat capacity of the material

ΔT = the temperature change

Data:

q = 2267 J

m = 44.5 g

T₁ = 33.9 °C

T₂ = 288.3 °C

Calculations:

ΔT = (288.3 - 33.9) °C = 254.4 °C

$\begin{array}{rcl}2267 & = & 44.5 \times C \times 254.4\\2267 & = & 11 180C\\C& = & \dfrac{2267}{11180}\\\\& = & \textbf{0.200 J$^{\circ}$C$^{-1}$g$^{-1}$}\\\end{array}$

$\text{The specific heat capacity of the metal is \boxed{\textbf{0.200 J$^{\circ}$C$^{-1}$g$^{-1}$}}}$

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4 years ago

To use combustion analysis data to determine an empirical formula A molecular formula expresses the number of each kind of atom

Kitty [74]

Answer:

0,1 mol of carbon and 0.2 moles of hydrogen were in the original sample.

Explanation:

The combustion reaction of the compound is

$C_{x} H_{y} O_{z} +O_{2} -> CO_{2} + H_{2}O$

And the molar mass of CO2 and H2O are 44g/mol and 18g/mol respectively

All the mass of carbon producing the CO2 must come from the carbon of the unknown compound, thus it is necessary to calculate the moles of carbon in 4.4g of CO2

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Also, all the mass of hydrogen producing the H2O must come from the hydrogen of the unknown compound, hence it is necessary to calculate the moles of hydrogen in 1.8g of water

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3 years ago