Ask question

Ask question

All categories

2 years ago

11

How would you describe the following chemical reaction?

1 answer:

GREYUIT [131]2 years ago

4 0

Answer:

B

Explanation:

The normal way to express an energy reaction is to put the energy on the left. Then you can make a rule.

If the energy on the left is plus then the reactants require energy. The reaction is endothermic -- energy is taken from the environment.
If the energy is minus when it is on the left. then the reactants give up energy. The reaction is exothermic and energy is given to the environment.

2CO(g)+O2(g) - energy --> 2CO2(g)

Exothermic

You might be interested in

An acid increases the hydroxide ion concentration of water.<br>True<br>or<br>False

ASHA 777 [7]

False is the answer!

3 0

2 years ago

Read 2 more answers

On a distance-time graph, at 2 hours the graph is at a height of 20 meters, and at 3 hours it is at a height of 100 meters. What

Gnoma [55]

Answer:

80 m/hr

Explanation:

Changes from 20 to 100 meters in ONE Hour

changes 80 meters in one hour = 80 m/hr

8 0

1 year ago

Who is telling what happens in Home Début?

nekit [7.7K]

Answer:

D

Explanation:

Its in first person

8 0

3 years ago

Consider the following chemical reaction: 2KCl + 3O2 --> 2KClO3. If you are given 100.0 moles of KCl and 100.0 moles of O2...

g100num [7]

Answer:

O₂; KCl; 33.3

Explanation:

We are given the moles of two reactants, so this is a limiting reactant problem.

We know that we will need moles, so, lets assemble all the data in one place.

2KCl + 3O₂ ⟶ 2KClO₃

n/mol: 100.0 100.0

1. Identify the limiting reactant

(a) Calculate the moles of KClO₃ that can be formed from each reactant

(i)From KCl

$\text{Moles of KClO}_{3} = \text{100.0 mol KCl} \times \dfrac{\text{2 mol KClO}_{3}}{\text{2 mol KCl}} = \text{100.0 mol KClO}_{3}$

(ii) From O₂

$\text{Moles of KClO}_{3} = \text{100.0 mol O}_{2} \times \dfrac{\text{2 mol KClO}_{3}}{\text{3 mol O}_{2}} = \text{66.67 mol KClO}_{3}$

O₂ is the limiting reactant, because it forms fewer moles of the KClO₃.

KClO₃ is the excess reactant.

2. Moles of KCl left over

(a) Moles of KCl used

$\text{Moles used} = \text{100.0 mol O}_{2} \times \dfrac{\text{2 mol KCl}}{\text{3 mol O}_{2}} = \text{66.67 mol KCl}$

(b) Moles of KCl left over

n = 100.0 mol - 66.67 mol = 33.3 mol

3 0

3 years ago

A patient needs to take 875mg twice daily The pills in the bottle are each 250mg How many pills does she wants to take 875mg

Angelina_Jolie [31]

Answer:

$3.5$ pill need to taken for completing dosage of $875$ mg

Explanation:

Total dosage of medicine to be taken in a day

$= 2 * 875 \\= 1750$ mg

Total weight of one pill $= 250$ mg

Number of pills required is equal to total dosage of medicine divided by the weight of one pill.

Hence,

Number of pills

$= \frac{875}{250} \\= \frac{175}{50} \\= \frac{35}{10} \\= 3.5$

6 0

3 years ago