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2 years ago

Which statement best describes a chemical property of Iron?

Chemistry

2 answers:

Karo-lina-s [1.5K]2 years ago

4 0

Answer:

I think it is iron conducts electricity and heat

mina [271]2 years ago

3 0

Answer:

C. Iron combines with oxygen to form rust.

Explanation:

The correct answer is "C" because it refers to the ability to rust, a chemical property, because rusting is a chemical change.

Answer choice "A" is incorrect because it refers to malleability, the ability to be flattened or pressed into sheets, a physical property. After being flattened, the iron would have gone through a physical change, not chemical.

Answer choice "B" is incorrect because it refers to conductivity, the ability to conduct electricity and heat, a physical property. The iron does not experience a chemical change while conducting.

Answer choice "D" is incorrect because it refers to ductility, the ability to be made into wire, a physical property. The iron is not going through a chemical change as wire.

You might be interested in

Ion Concentration 1. Which solution has the greatest [SO42-]: a) 0.075 M H2SO4 b) 0.15 M Na2SO4 c) 0.080 M Al2(SO4)3?

soldi70 [24.7K]

Answer:

c) 0.080 M Al₂(SO₄)₃

Explanation:

Ion [SO₄²⁻] concentration of each solution is:

a) 0.075 M H₂SO₄: [SO₄²⁻] = 0.075M. Because 1 mole of H₂SO₄ contains 1 mole of SO₄²⁻

b) 0.15 M Na₂SO₄: [SO₄²⁻] = 0.15M. Also, 1 mole of Na₂SO₄ contains 1 mole of SO₄²⁻

c) 0.080 M Al₂(SO₄)₃ [SO₄²⁻] = 0.080Mₓ3 = 0.240M. Because 1 mole of Al₂(SO₄)₃ contains 3 moles of SO₄²⁻.

<h3>Thus, the soluion that has the greatest [SO₄²⁻] is 0.080 M Al₂(SO₄)₃</h3>

8 0

3 years ago

How much energy is released by the decay of 3 grams of 230Th in the following reaction 230 Th - 226Ra + "He (230 Th = 229.9837 g

Serhud [2]

Answer: The energy released for the decay of 3 grams of 230-Thorium is $2.728\times 10^{-15}J$

Explanation:

First we have to calculate the mass defect $(\Delta m)$ .

The equation for the alpha decay of thorium nucleus follows:

$_{90}^{230}\textrm{Th}\rightarrow _{88}^{226}\textrm{Ra}+_2^{4}\textrm{He}$

To calculate the mass defect, we use the equation:

Mass defect = Sum of mass of product - Sum of mass of reactant

$\Delta m=(m_{Ra}+m_{He})-(m_{Th})$

$\Delta m=(225.9771+4.008)-(229.9837)=1.4\times 10^{-3}amu=2.324\times 10^{-30}kg$

(Conversion factor: $1amu=1.66\times 10^{-27}kg$ )

To calculate the energy released, we use Einstein equation, which is:

$E=\Delta mc^2$

$E=(2.324\times 10^{-30}kg)\times (3\times 10^8m/s)^2$

$E=2.0916\times 10^{-13}J$

The energy released for 230 grams of decay of thorium is $2.0916\times 10^{-13}J$

We need to calculate the energy released for the decay of 3 grams of thorium. By applying unitary method, we get:

As, 230 grams of Th release energy of = $2.0916\times 10^{-13}J$

Then, 3 grams of Th will release energy of = $\frac{2.0916\times 10^{-13}}{230}\times 3=2.728\times 10^{-15}J$

Hence, the energy released for the decay of 3 grams of 230-Thorium is $2.728\times 10^{-15}J$

5 0

3 years ago

Is the formation of acid rain an exothermic or endothermic reaction?

Monica [59]

It is an exothermic reaction

4 0

3 years ago

What mass of H2 is needed to react with 8.75 g of O2 according to the following equation: O2(g) + H2(g) → H2O(g)?

Alika [10]

Answer:- B: $1.10g H_2$ is the right answer.

Solution:- The balanced equation is:

$O_2(g)+2H_2(g)\rightarrow 2H_2O(g)$

We have been given with 8.75 grams of oxygen and asked to calculate the grams of hydrogen needed to react with given grams of oxygen according to the balanced equation.

From balanced equation, 1 mole of oxygen reacts with 2 moles of hydrogen.

So, let's convert grams of oxygen to moles and multiply it by the mole ratio to calculate the moles of hydrogen that are easily converted to grams on multiplying by it's molar mass.

The complete set up looks as:

$8.75g O_2(\frac{1mole}{32g})(\frac{2mole H_2}{1mole O_2})(\frac{2.02g}{1mole})$

= $1.10g H_2$

Hence, the right option is B: $1.10g H_2$ .

7 0

3 years ago

Read 2 more answers

Identify the number of moles in 369 grams of calcium hydroxide. Use the periodic table and the polyatomic ion resource.

topjm [15]

Answer : The number of moles in 369 grams of calcium hydroxide is, 4.98 moles

Explanation : Given,

Mass of calcium hydroxide = 369 g

Molar mass of calcium hydroxide = 74.093 g/mole

Formula used :

$\text{Moles of calcium hydroxide}=\frac{\text{Mass of calcium hydroxide}}{\text{Molar mass of calcium hydroxide}}$

Now put all the given values in this formula, we get the moles of calcium hydroxide.

$\text{Moles of calcium hydroxide}=\frac{369g}{74.093g/mole}=4.98mole$

Therefore, the number of moles in 369 grams of calcium hydroxide is, 4.98 moles

7 0

3 years ago