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3 years ago

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A piece of iron at 75.0oC is dropped into 50.0 g of water at 20.0oC. The final temperature of the water is 28.3oC. The specific

heat of iron is 0.450 j/goC. Determine the mass of the piece of iron.

1 answer:

AleksandrR [38]3 years ago

5 0

Answer:

<h2>13</h2>

Explanation:

<em>b</em><em>e</em><em> </em><em>c</em><em>r</em><em>i</em><em>t</em><em>i</em><em>c</em><em>a</em><em>l</em><em> </em><em>t</em><em>h</em><em>i</em><em>n</em><em>k</em><em>e</em><em>r</em><em>s</em>

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In the reaction between bromine and sodium, a bromine atom gains an electron and forms the bromide ion, Br-. What happens to bro

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It becomes ionized and attains its stable electronic configuration.

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3 years ago

HELP WITH THIS ASAP PLEASE!!! What is the mass in grams of 8.42 x 10^22 atoms of sulfur?

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Answer:

Answer:

see explanation and punch in the numbers yourself ( will be better for your test)

Explanation:

If you are given atoms you need to divide by Avogadro's number 6.022x10^23

then you will have moles of sulfur-- once you have moles multiply by the molar mass of sulfur to go from moles to grams

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3 years ago

Difference between proton and electron

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Answer:

An electron is a negatively charged component of an atom

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3 years ago

How many grams of XeF6 are required to react with 0.579 L of hydrogen gas at 4.46 atm and 45°C in the reaction shown below?

natka813 [3]

Answer:

8.1433 g of XeF₆ are required.

Explanation:

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Given data:

Volume of hydrogen = 0.579 L

Pressure = 4.46 atm

Temperature = 45 °C (45+273= 318 k)

Solution:

First of all we will calculate the moles of hydrogen

PV = nRT

n = PV/ RT

n = 4.46 atm × 0.579 L / 0.0821 atm. dm³. mol⁻¹. K⁻¹ × 318 K

n = 2.6 atm . L / 26.12 atm. dm³. mol⁻¹

n = 0.0995 mol

Mass of hydrogen:

Mass = moles × molar mass

Mass = 0.0995 mol × 2.016 g/mol

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Now we will compare the moles of hydrogen with XeF₆ from balance chemical equation.

H₂ : XeF₆

3 : 1

0.0995 : 1/3× 0.0995 = 0.0332 mol

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3 years ago

Give the Unabbreviated electron configuration for barium

Shalnov [3]

Answer:

Ba: 1s² 2s²2p⁶ 3s²3p⁶ 4s²3d¹⁰4p⁶ 5s²4d¹⁰5p⁶ 6s²

Step-by-step explanation:

Step 1. Locate barium in the Periodic Table.

It's in Period 6, Group 2: Element 56 (highlighted blue in the Periodic Table below).

Step 2. Add 54 electrons to the energy levels

You add then in the order shown in the diagram below.

The complete electron configuration is:

Ba: 1s² 2s²2p⁶ 3s²3p⁶ 4s²3d¹⁰4p⁶ 5s²4d¹⁰5p⁶ 6s²

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8 0

3 years ago