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soldi70 [24.7K]
3 years ago
12

Which is the isoelectronic of Na​

Chemistry
1 answer:
postnew [5]3 years ago
6 0

Mg- is the isoelectronic of Na

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What part of the microscope is the letter k?
snow_tiger [21]

Answer:

if you are asking k then the round one is condenser

if not then its a stage clip

6 0
2 years ago
Balance the following Chemical Equation:<br> NaBr +CaCl2-&gt; NaCl+ CaBr2
frozen [14]
First write all of the compounds/atoms in either side then fill in existing values and balance


Na- 1
Br- 1
Ca- 1
Cl- 2

Na- 1
Cl- 1
Ca-1
Br-2

Balance to get

2NaBr+CaCl2=2NaCl+CaBr2
7 0
2 years ago
Given the following equation: 2K + Cl2 -&gt; 2KCl How many grams of KCl is produced from 4.00 g of K and excess Cl2?
Thepotemich [5.8K]

Answer:

42.65g

Explanation:

Given parameters:

Mass of K = 4g

Unknown: Mass of KCl

Solution:

  Complete equation of the reaction:

              2K + Cl₂ → 2KCl

To solve this problem, we know that the reactant in short supply is potassium K and this dictates the amount of products that would be formed. The chlorine gas is in excess and we can't use it to determine the amount of product that would form.

Now, we work from the known to the unknown. Since we know the mass of K given in the reaction, we can simply find the molar relationship between the reacting potassium and the product. We simply convert the mass to mole and compare to the product. From there we can find the mass of KCl that would be produced.

Calculating number of moles of K

      Number of moles = \frac{mass}{molar mass}

        Number of moles of K =  \frac{4}{39} = 0.103mol

From the given reaction equation:

   2 moles of K will produce 2 moles of KCl

 Therefore 0.103mol of K will produce 0.103mol of KCl

To find the mass of KCl produced,

   Mass of KCl = number of moles of KCl x molar mass

Molar mass of KCl = 39 + 35.5 = 74.5gmol⁻¹

Mass of KCl = 0.103 x 74.5 = 42.65g

4 0
3 years ago
Read 2 more answers
Breaking down earths surface
tino4ka555 [31]

☁️ Answer ☁️

Thats called weathering.

Weathering describes the breaking down or dissolving of rocks and minerals on the surface of the Earth.

Hope it helps.

Have a nice day noona/hyung!~  ̄▽ ̄❤️

6 0
2 years ago
An experiment shows that a 236 mL gas sample has a mass of 0.443 g at a pressure of 740 mmHg and a temperature of 22 ∘C. What is
aleksley [76]

Answer:

49.2 g/mol

Explanation:

Let's first take account of what we have and convert them into the correct units.

Volume= 236 mL x (\frac{1 L}{1000 mL}) = .236 L

Pressure= 740 mm Hg x (\frac{1 atm}{760 mm Hg})= 0.97 atm

Temperature= 22C + 273= 295 K

mass= 0.443 g

Molar mass is in grams per mole, or MM= \frac{mass}{moles} or MM= \frac{m}{n}. They're all the same.

We have mass (0.443 g) we just need moles. We can find moles with the ideal gas constant PV=nRT. We want to solve for n, so we'll rearrange it to be

n=\frac{PV}{RT}, where R (constant)= 0.082 L atm mol-1 K-1

Let's plug in what we know.

n=\frac{(0.97 atm)(0.236 L)}{(0.082)(295K)}

n= 0.009 mol

Let's look back at MM= \frac{m}{n} and plug in what we know.

MM= \frac{0.443 g}{0.009 mol}

MM= 49.2 g/mol

3 0
2 years ago
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