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3 years ago

Help me with this please I need the answers ASAP

Chemistry

1 answer:

Tema [17]3 years ago

7 0

Answer:

1. Exothermic reaction

2. Is being released

3. The energy comes from the change in energy between reactants and products

Explanation:

The reaction is producing energy. A reaction that produce energy is called a <em>Exothermic reaction.</em>

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As the energy is produced, the energy is being <em>released.</em>

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As you can see in the image, the energy of the reactants is higher than the energy of the products. This change of energy in the chemicals produce the production of energy as heat.

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Table of ions *chemistry* Please Help me

Elza [17]

Answer:

See Attached Table

Explanation:

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3 years ago

Given the equation representing a reaction at equilibrium: h2s(aq) ch3nh2(aq) hs(aq) ch3nh3 (aq) according to one acid-base theo

alekssr [168]

Since in the forward reaction, H2S is giving a proton away (being the acid) and then CH3NH2 accepting that proton given (being the base).

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4 years ago

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What is neutral subatomic particles

AleksAgata [21]

Answer:

<h3>Neutron, neutral subatomic particle that is a constituent of every atomic nucleus except ordinary hydrogen</h3>

Explanation:

<h3>hope it helps u..</h3>

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3 years ago

22 g de um gás estão contidos em um recipiente de volume igual a 17,5 L, a uma temperatura de 77ºC e

Aleksandr-060686 [28]

Answer:

Option D.

Explanation:

Let's apply the Ideal Gases law to solve the problem.

P . V = n . R . T

First of all we convert the temperature value from °C to K

77°C + 273 = 350K

and the pressure from mmHg to atm

623 mmHg . 1 atm/760 mmHg = 0.82 atm

We replace data: 0.82 atm . 17.5L = n . 0.082 L.atm/mol.K . 350K

(0.82 atm . 17.5L) / (0.082 L.atm/mol.K . 350K) = n

0.50 moles = n

These are the moles that corresponds to 22 g of the gas, so the molar mass will be → 22g / 0.50 mol = 44 g/mol

That molar mass corresponds to CO₂ → 12 g (C) + 16 g (O) . 2 = 44 g/mol

4 0

3 years ago

Please help!!!!! I need the correct answer quickly!!!

xxMikexx [17]

Answer :

The oxidation state of oxygen (O) in $OF_2$ is, (+2)

The oxidation state of carbon (C) in $CO$ is, (+2)

The oxidation state of nitrogen (N) in $K_3N$ is, (-3)

Explanation :

Oxidation number : It represent the number of electrons lost or gained by the atoms of an element in a compound.

Oxidation numbers are generally written with the sign (+) and (-) first and then the magnitude.

When the atoms are present in their elemental state then the oxidation number will be zero.

Rules for Oxidation Numbers :

The oxidation number of a free element is always zero.

The oxidation number of a monatomic ion equals the charge of the ion.

The oxidation number of Hydrogen (H) is +1, but it is -1 in when combined with less electronegative elements.

The oxidation number of oxygen (O) in compounds is usually -2, but it is -1 in peroxides.

The oxidation number of a Group 1 element in a compound is +1.

The oxidation number of a Group 2 element in a compound is +2.

The oxidation number of a Group 17 element in a binary compound is -1.

The sum of the oxidation numbers of all of the atoms in a neutral compound is zero.

The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

(a) The given compound is, $OF_2$

Let the oxidation state of 'O' be, 'x'

$x+2(-1)=0\\\\x-2=0\\\\x=+2$

The oxidation state of oxygen (O) in $OF_2$ is, (+2)

(b) The given compound is, $CO$

Let the oxidation state of 'C' be, 'x'

$x+(-2)=0\\\\x-2=0\\\\x=+2$

The oxidation state of carbon (C) in $CO$ is, (+2)

(c) The given compound is, $K_3N$

Let the oxidation state of 'N' be, 'x'

$3(+1)+x=0\\\\3+x=0\\\\x=-3$

The oxidation state of nitrogen (N) in $K_3N$ is, (-3)

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3 years ago

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