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4 years ago

Which statement about exothermic reactions is accurate?

Chemistry

2 answers:

frosja888 [35]4 years ago

6 0

Answer:

A) As reactants form products, the potential energy decreases.

Explanation:

this is correct on ed-genuity, hope this helps! :)

ki77a [65]4 years ago

4 0

Answer is: As reactants form products, the potential energy decreases.

There are two types of reaction:

1) Endothermic reaction (chemical reaction that absorbs more energy than it releases).

2) Exothermic reaction (chemical reaction that releases more energy than it absorbs).

For example, balanced chemical reaction:

C₂H₅OH + 3O₂ → 2CO₂ + 3H₂O ΔrH= -1370 kJ/mol.

This reaction is exothermic reaction (heat is released), so products have less potential energy and energy is transerred to surroundings.

You might be interested in

What is the mass in grams of 9.76 × 1012 atoms of naturally occurring beryllium?

Ksivusya [100]

The atomic mass of beryllium (Be) is 9 g/mole

Now, 1 mole of any substance contains avogadro's number of that substance. Therefore:

1 mole of Be contains 6.023 10^23 atoms of Be

In other words:

9 grams of Be contains 6.023*10^23 atoms of Be

Therefore, the mass corresponding to 9.76 * 10^12 atoms of Be is:

= 9 g * 9.76 10^12 atoms/6.023*10^23 atoms

= 1.458 * 10^-10 g (or) 1.46 * 10^-10 g

8 0

3 years ago

Read 2 more answers

What is the formula,molecular geometry,and bonding angle for ch2ci

stellarik [79]

Answer:

what

Explanation:

6 0

3 years ago

For a reaction in a galvanic cell both ΔH° and ΔS° are positive. Which of the following statements is true?

irina [24]

Answer:

Option C is the correct statement.

ℰ°cell will increase with an increase in temperature

Explanation:

To understand this problem it is neccessarry to state the relatioonships between the various paramenters mentioned in the question. these parameters include ΔH°, ΔS°, ΔG° and ℰ°Cell.

ΔH°, ΔS°, ΔG° are related with the following equation;

ΔG° = ΔH° - TΔS°

From the above equation we see that ΔG° cannot be greater than 0 for all temperatures. At higher temperatures, ΔG° becomes a negative value.

A spontaneous redox reaction is characterized by a negative value of ΔG and a positive value of ℰ°Cell, consistent with our earlier discussions. When both reactants and products are in their standard states, the relationship between ΔG° and ℰ°Cell is as follows:

ΔG∘=−nFℰ°Cell where;

F = Faraday and n = number of moles

Since ΔG° becomes negative at higher temperatures, it means ℰ°Cell would increase as temperature increases.

The relationship between G, Ecell and temperature can be given as;

Increase in Temperature = Negative value of G = Increase in E

Due to the fact established above; options B, D and E are false. This means the correct option is option C - ℰ°cell will increase with an increase in temperature

3 0

3 years ago

The human body needs at least 1.03 x 10-^2 mol O2 every minute. If all of this oxygen is used for the

Neko [114]

<h3>Answer:</h3>

0.3093 g of glucose are consumed each minute by the body.

<h3>Explanation:</h3>

During cellular respiration glucose is broken down in presence of oxygen to yield energy, water and carbon dioxide.
The equation for the reaction taking place during cellular respiration is;

C₆H₁₂O₆ + 6O₂ → 6H₂O + 6CO₂

We are required to calculate the amount of glucose in grams;

<h3>Step 1: Calculate the moles of glucose broken down</h3>

From the equation, the mole ratio of glucose to Oxygen is 1 : 6

Moles of Oxygen in a minute is 1.03 × 10^-2 moles

Therefore, moles of glucose will be;

= (1.03 × 10^-2)÷6

= 1.717 × 10^-3 moles

<h3>Step 2: Mass of glucose </h3>

Mass is given by multiplying the number of moles with molar mass

mass = moles × molar mass

Molar mass glucose is 180.156 g/mol

Therefore;

Mass = 1.717 × 10^-3 × 180.156 g/mol

= 0.3093 g

Hence, 0.3093 g of glucose are consumed each minute by the body.

3 0

4 years ago

1) How many atoms are in 0.54 moles of Cu? show work

mario62 [17]

<h3>Answer:</h3>

3.3 × 10²³ atoms Cu

<h3>General Formulas and Concepts:</h3>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right<u> </u>

<u>Chemistry</u>

<u>Atomic Structure</u>

Moles
Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<u>Stoichiometry</u>

Using Dimensional Analysis

<h3>Explanation:</h3>

<u>Step 1: Define</u>

[Given] 0.54 moles Cu

[Solve] atoms Cu

<u>Step 2: Identify Conversions</u>

Avogadro's Number

<u>Step 3: Convert</u>

[DA] Set up: $\displaystyle 0.54 \ mol \ Cu(\frac{6.022 \cdot 10^{23} \ atoms \ Cu}{1 \ mol \ Cu})$
[DA] Multiply [Cancel out units]: $\displaystyle 3.25188 \cdot 10^{23} \ atoms \ Cu$

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 2 sig figs.</em>

3.25188 × 10²³ atoms Cu ≈ 3.3 × 10²³ atoms Cu

7 0

3 years ago