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2 years ago

Isotopes are different types of atoms of the same element, but with a different number of __________ ?

Chemistry

2 answers:

rodikova [14]2 years ago

6 0

Same things but with different numbers of neutrons in nuclei

bija089 [108]2 years ago

4 0

Answer:

A different atomic mass, which means that there is a varying number of nuetrons in the nucleus between isotopes.

Explanation:

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What is the shorthand electron configuration for Ba2+

Arada [10]

Since the barium ion will be isoelectronic to the nearest noble gas, which is xenon, the electronic configuration for Ba2+ is: [Xe]

3 0

3 years ago

300 moles of sodium nitrite are needed for a reaction. the solution is 0.450 m. how many ml are needed?

miv72 [106K]

Answer:

$\boxed{\text{667 000 mL}}$

Explanation:

$\text{Molar concentration} = \dfrac{\text{moles}}{\text{litres}}\\\\c = \dfrac{n}{v}$

Data:

c = 0.450 mol·L⁻¹

n = 300 mol

Calculation:

$\begin{array}{rcl}0.450 & = & \dfrac{300}{V}\\\\0.450V& = & 300\\\\V & = & \dfrac{300}{0.450}\\\\V & = & \text{667 L} =\textbf{667 000 mL}\end{array}\\\text{The volume of solution needed is }\boxed{\textbf{667 000 mL}}$

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3 years ago

What type of reaction does this equation represent?

bonufazy [111]

Answer:

$its \: d. \: double \: replacement \: .$

Explanation:

$hope \: it \: helps \: out \:$

4 0

3 years ago

To make a 6.50M solution, how many moles of solute will be needed if 12.0 liters of solution are required

avanturin [10]

Answer:

78 moles of the solute

Explanation:

From the question;

Molarity of the solution is 6.50 M
Volume of the solution is 12.0 L

We want to determine the number of moles needed

We need to know that;

Molarity = Number of moles ÷ Volume

Therefore;

Number of moles = Molarity × Volume

Hence;

Number of moles = 6.50 M × 12.0 L

= 78 moles

Thus, the moles of the solute needed is 78 moles

8 0

3 years ago

Consider the following reversible reaction N2 + 3H2 = 2NH, In a 3 L container, the following amounts are found in equilibrium at

dolphi86 [110]

769km - grams 60000 *

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2 years ago