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3 years ago

Two different liquids are mixed together. Which observation indicates that an exothermic chemical reaction has taken place?

2 answers:

8 0

Well for one, A LOT of heat (or if you wanna call it energy) is being released from the mixture and the container itself starts to heat up and you can DEFINITELY feel the heat. EXO: Outside, exterior. THERMIC: Heat, something to describe hot stuff (I guess).

SO you can say it heats up the outside container and occasionally will produce steam or foam (DEPENDING ON WHAT YOU MIX)

fenix001 [56]3 years ago

4 0

your answer is: a rise in temperature

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Does iron always have a charge of 2+ when it forms an ion

Usimov [2.4K]

Answer:

Roman numeral notation indicates charge of ion when element commonly forms more than one ion. For example, iron(II) has a 2+ charge; iron(III) a 3+ charge.

Explanation:

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3 years ago

If you have a pitcher of lemonade and the recipe calls for 2 lemons and you decided to use 4, would this be considered diluted o

pantera1 [17]

Answer: This would be considered concentrated because if you're upping the recipe on your own accord, it would be way more sour, causing the lemonade to be more concentrated. It would be diluted if you added less than 2 lemons.

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3 years ago

Briefly discuss interpretations of your observations and results. Discuss how your observations illustrated LeChatelier's princi

Dvinal [7]

Answer:

Le Chatelier's principle can be applied in explaining the results

Explanation:

According to Le Chatelier's principle, when a constraint such as a change in concentration in this case is imposed on a chemical system in equilibrium, the system will adjust itself in such a way as to annul the constraint imposed.

Hence, when the color of the solution was more like that of the control, the reaction would shift towards the left. Similarly, when the color was more like it was towards the reactant, the reaction would shift towards the right.

If we were to prepare calcium oxalate, we should prepare it in a base solution. This is because when the base was added to calcium oxalate, it did not form any precipitate but when an acid was added to the calcium oxalate, it formed a precipitate.

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2 years ago

a technician mixes 80 ml of a 5% solution with 10 ml of water. what is the final percentage strength of the solution prepared?

Vinvika [58]

A technician mixes 80 ml of a 5% solution with 10 ml of water. the final percentage strength of the solution prepared is 40 %.

given that :

8 ml of a 5 % solution mix with 10 ml . that means the 80 mL of 5 % solution is diluted with water of 10 mL

therefore, 80 × 5 = 10 × x %

x % = 40 %

Therefore, the final percentage strength of the solution is 40 %

Thus, A technician mixes 80 ml of a 5% solution with 10 ml of water. the final percentage strength of the solution prepared is 40 %.

To learn more about percentage strength here

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1 year ago

Be sure to answer all parts. Express the rate of reaction in terms of the change in concentration of each of the reactants and p

Tanzania [10]

Answer : The [H] is increasing at the rate of 0.36 mol/L.s

Explanation :

The general rate of reaction is,

$aA+bB\rightarrow cC+dD$

Rate of reaction : It is defined as the change in the concentration of any one of the reactants or products per unit time.

The expression for rate of reaction will be :

$\text{Rate of disappearance of A}=-\frac{1}{a}\frac{d[A]}{dt}$

$\text{Rate of disappearance of B}=-\frac{1}{b}\frac{d[B]}{dt}$

$\text{Rate of formation of C}=+\frac{1}{c}\frac{d[C]}{dt}$

$\text{Rate of formation of D}=+\frac{1}{d}\frac{d[D]}{dt}$

$Rate=-\frac{1}{a}\frac{d[A]}{dt}=-\frac{1}{b}\frac{d[B]}{dt}=+\frac{1}{c}\frac{d[C]}{dt}=+\frac{1}{d}\frac{d[D]}{dt}$

From this we conclude that,

In the rate of reaction, A and B are the reactants and C and D are the products.

a, b, c and d are the stoichiometric coefficient of A, B, C and D respectively.

The negative sign along with the reactant terms is used simply to show that the concentration of the reactant is decreasing and positive sign along with the product terms is used simply to show that the concentration of the product is increasing.

The given rate of reaction is,

$2D(g)+3E(g)+F(g)\rightarrow 2G(g)+H(g)$