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3 years ago

Help, please X﹏X- The picture in the right is after the water drained out -

Chemistry

2 answers:

lutik1710 [3]3 years ago

6 0

There’s no picture in your question

ioda3 years ago

6 0

Answer:

a or c

Explanation:

Can I have the brainliest pls?

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Calculate the mass in grams of carbon needed to produce 160 g of CO2 in burning: C + O2 --> CO2

Vladimir [108]

160gof CO2×1molof CO2\44g of CO2×1mole of C\1mol of CO2×12g of C\1mole of C=
43.63g of C

5 0

3 years ago

What is the pH of a solution with a 3.2 x 10−6 M hydronium ion concentration?

Rainbow [258]

Answer:

Explanation:

The pH of a solution can be found by using the formula

$pH = - log ([ { H_3O}^{+}])$

H3O+ is the hydronium ion

From the question we have

$pH = - log(3.2 \times {10}^{ - 6} ) \\ = 5.49485..$

We have the final answer as

Hope this helps you

4 0

3 years ago

How do you correctly put the number 0.00000000008759 in scientific notation with 3 sig figs?

vesna_86 [32]

Answer:

8.759×10-11

Explanation:

it may be to sure try to convert the answer

5 0

3 years ago

In a certain chemical reaction Compound A combines with Compound B to produce Compound C (and no other products). Measurements w

Karo-lina-s [1.5K]

Answer:

Theoretical yield of C = 7.9 g

Actual amount of C isolated = 5.0 g

Explanation:

Given that in the reaction, Compound A combines with Compound B t o produce Compound C and no other products, the reaction is a combination reaction. The equation of the reaction is given below:

A + B ---> C

Part A:

From the measurement of the masses of A and B present before and after the reaction, the following values were obtained:

Initial mass of A = 4.0 g

Final mass of A = 0.0 g

Mass of A used up + 4.0 - 0.0 = 4.0 g

Initial mass of B = 9.0 g

Final mass of B = 5.1 g

Mass of B used up = 9.0 - 5.1 = 3.9 g

According to the law of conservation of mass, matter can neither be created nor destroyed but can change from one form to another. Therefore, theoretical yield of C equal the sum of the masses of A and B used up.

Theoretical yield of C = 4.0 + 3.9 = 7.9 g

Part B:

Given that the percent yield is 63.0 % = 0.63

Actual amount of C isolated = 0.63 * 7.9 = 5.0 g

5 0

3 years ago

You've just solved a problem and the answer is the mass of an electron, me=9.11×10−31kilograms. How would you enter this number

mihalych1998 [28]

The mass of an electron can be expressed in the box as $\boxed{{m_e} = 9.1 \times {{10}^{ - 31}}{\text{ kg}}}$ .

Further explanation:

Atom is the smallest particle that can be present in any element. It is also known as the building unit of matter. Each atom has a central part that is known as the atomic nucleus. There are three subatomic particles that constitute the atom. These particles are protons, neutrons, and electrons. The atomic nucleus consists of protons and neutrons, both are collectively called nucleons. Electrons revolve around the nucleus of an atom in definite orbits.

Protons are positively charged subatomic particles, electrons are negatively charged and neutrons have no charge. Since electrons carry a unit negative charge, these create an electric field around them. These also participate in nuclear reactions. The mass of an electron $\left( {{m_e}} \right)$ is $9.1 \times {10^{ - 31}}{\text{ kg}}$ , that of protons is $1.6726219 \times {10^{ - 27}}{\text{ kg}}$ and that of neutrons is $1.674927471 \times {10^{ - 27}}{\text{ kg}}$ . The electrons are responsible for chemical properties of elements. The distribution and arrangement of electrons is used to predict whether the element will be inert or reactive.

Therefore the required answer is $\boxed{{m_e} = 9.1 \times {{10}^{ - 31}}{\text{ kg}}}$ .

Learn more:

Component of John Dalton’s atomic theory: brainly.com/question/2357175
Basis of investigation for the scientists: brainly.com/question/158048

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Atomic structure

Keywords: atom, matter, atomic nucleus, proton, electron, neutron, subatomic particle, nuclear reactions, electric field, reactive, inert.

4 0

4 years ago