:

Name the components of an atom which determines each of the following

bulgar [2K]

Answer:

answer is Proton.

Explanation:

because electron is too heavy and other one has no charge

4 0

3 years ago

Convert 7.2 × 10^23 molecules of CO2 to moles (round to the nearest tenth). <br>Unit?

Svetach [21]

7.2 * 10^23 molecules CO2 1 mole CO2

x ___________________

6.02* 10^23 molecules CO2

=1.196

=1.2 moles of CO2

5 0

3 years ago

Find the empirical formula of the following compounds:

Aneli [31]

The empirical formula of the following compounds 0.903 g of phosphorus combined with 6.99 g of bromine.

<h3>What is empirical formula?</h3>

The simplest whole number ratio of atoms in a compound is the empirical formula of a chemical compound in chemistry. Sulfur monoxide's empirical formula, SO, and disulfur dioxide's empirical formula, S2O2, are two straightforward examples of this idea. As a result, both the sulfur and oxygen compounds sulfur monoxide and disulfur dioxide have the same empirical formula.

<h3>How to find the empirical formula?</h3>

Convert the given masses of phosphorus and bromine into moles by multiplying the reciprocal of their molar masses. The molar masses of phosphorus and bromine are 30.97 and 79.90 g/mol, respectively.

Moles phosphorus = 0.903 g phosphorus $\frac{mol phosphorus}{ 30.97 g phosphorus}$ = 0.0293 mol

Moles bromine 6.99 g bromine $\frac{mol bromine}{79.90 g bromine}$ =0.0875 mol

The preliminary formula for compound is P0.0293Bro.0875. Divide all the subscripts by the subscript with the smallest value which is 0.0293. The empirical formula is P1.00Br2.99 ≈ P₁Br3 or PBr3

To learn more about empirical formula visit:

brainly.com/question/14044066

#SPJ4

8 0

1 year ago

Stoichiometry Problems!

lisov135 [29]

Hey there!

C₆H₁₂O₆(s) + 6O₂(g) => 6CO₂(g) + 6H₂0(l)

a.)

First we need to find how many molecules of oxygen gas we need.

Every one molecule of C₆H₁₂O₆ will react with six molecules of O₂. So, if we have 3.011 x 10²³ molecules of C₆H₁₂O₆, we need six times that of oxygen.

3.011 x 10²³ x 6 = 18.066 x 10²³ = 1.8066 x 10²⁴

So we need 1.8066 x 10²⁴ molecules of O₂. We need to find the volume of this in liters.

At STP, one mole of a gas occupies 22.4 liters. Let's find the number of moles we have of O₂.

(1.8066 x 10²⁴) ÷ (6.022 x 10²³) = 3 moles

3 x 22.4 = 67.2

67.2 liters of O₂ is needed.

b.)

Okay, so to find the percent yield, we need to find the theoretical yield and the actual yield. We are given the actual yield, so what we need is the theoretical yield.

For every one mole of C₆H₁₂O₆, theoretically 6 moles of H₂O will be produced.

Let's convert grams to moles for C₆H₁₂O₆:

1 gram / 180 grams = 0.0055556 moles C₆H₁₂O₆

Theoretically, 6 times that is the moles of H₂O produced:

0.0055556 x 6 = 0.033333 moles H₂O

Molar mass of H₂O is 18.015, so let's find grams:

0.033333 x 18.015 = 0.600 grams H₂O

So we have our theoretical yield, 0.600, and our actual yield, 0.303.

0.303 ÷ 0.600 = 0.505

Convert to a percent: 0.505 x 100 = 50.5%

The percent yield is 50.5%.

Hope this helps!

4 0

3 years ago

Place the following elements of the scale below from lowest energy ties energy

BARSIC [14]

Li, Na, K, Ca, Fe, Cu, Sr

7 0

3 years ago