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4 years ago

The rate of the reaction is ?

2 answers:

4 0

The rate of a chemical reaction is defined as the change in the concentration of a reactant or a product over the change in time, and concentration is in moles per liter, or molar, and time is in seconds. So we express the rate of a chemical reaction in molar per second.

IRISSAK [1]4 years ago

3 0

Answer:

Hey!

Your answer is The Rate of a Reaction is a measurement of how the speed at which a reactant is used up / or a product is formed.

Explanation:

R of R (Rate of Reaction) can be affected by:

Reactant concentration (how much of the substance is there to react)

The state of the reactants (whether they are in a solid/liquid/gas state)

The total surface area (more particles of the substance means more reactions...)

The Temperature (hot=quicker cool=slower)

The presence of a catalyst (catalysts speed up the Rate of the Reaction)

HOPE THIS HELPS!!

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How many grams of sodium hydroxide are needed to completely react with 50.0 grams of H2SO4?

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48.0 grams of NaOH I believe

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3 years ago

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How many moles are in 1.806 x 1024 molecules of bromine?

Pepsi [2]

<h3>Answer:</h3>

2.999 mol Br

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

<u>Math</u>

<u>Pre-Algebra</u>

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Parenthesis
Exponents
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Left to Right

<u>Chemistry</u>

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Using Dimensional Analysis
Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<h3>Explanation:</h3>

<u>Step 1: Define</u>

1.806 × 10²⁴ molecules Br

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

Avogadro's Number

<u>Step 3: Convert</u>

<u /> $\displaystyle 1.806 \cdot 10^{24} \ molecules \ Br(\frac{1 \ mol \ Br}{6.022 \cdot 10^{23} \ molecules \ Br} )$ = 2.999 mol Br

<u>Step 4: Check</u>

<em>We are given 4 sig figs. Follow sig fig rules and round.</em>

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3 years ago

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Explain how mary would conduct a science experiment to test wheather plants need soil to grow.

Elis [28]

Try to grow a plant with and without soil

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3 years ago

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Consider the following reaction at a high temperature. Br2(g) ⇆ 2Br(g) When 1.35 moles of Br2 are put in a 0.780−L flask, 3.60 p

UNO [17]

Answer : The equilibrium constant $K_c$ for the reaction is, 0.1133

Explanation :

First we have to calculate the concentration of $Br_2$ .

$\text{Concentration of }Br_2=\frac{\text{Moles of }Br_2}{\text{Volume of solution}}$

$\text{Concentration of }Br_2=\frac{1.35moles}{0.780L}=1.731M$

Now we have to calculate the dissociated concentration of $Br_2$ .

The balanced equilibrium reaction is,

$Br_2(g)\rightleftharpoons 2Br(aq)$

Initial conc. 1.731 M 0

At eqm. conc. (1.731-x) (2x) M

As we are given,

The percent of dissociation of $Br_2$ = $\alpha$ = 1.2 %

So, the dissociate concentration of $Br_2$ = $C\alpha=1.731M\times \frac{1.2}{100}=0.2077M$

The value of x = 0.2077 M

Now we have to calculate the concentration of $Br_2\text{ and }Br$ at equilibrium.

Concentration of $Br_2$ = 1.731 - x = 1.731 - 0.2077 = 1.5233 M

Concentration of $Br$ = 2x = 2 × 0.2077 = 0.4154 M

Now we have to calculate the equilibrium constant for the reaction.

The expression of equilibrium constant for the reaction will be :

$K_c=\frac{[Br]^2}{[Br_2]}$

Now put all the values in this expression, we get :

$K_c=\frac{(0.4154)^2}{1.5233}=0.1133$

Therefore, the equilibrium constant $K_c$ for the reaction is, 0.1133

7 0

3 years ago

Calculate the number of calories needed to increase the temperature of 50.0 g of copper metal from 21.0 degrees C to 75.0 degree

KonstantinChe [14]

<h3>Answer:</h3>

1031.4 Calories.

<h3>Explanation:</h3>

We are given;

Mass of the copper metal = 50.0 g

Initial temperature = 21.0 °C

Final temperature, = 75°C

Change in temperature = 54°C

Specific heat capacity of copper = 0.382 Cal/g°C

We are required to calculate the amount of heat in calories required to raise the temperature of the copper metal;

Quantity of heat is given by the formula,

Q = Mass × specific heat capacity × change in temperature

= 50.0 g × 0.382 Cal/g°C × 54 °C

= 1031.4 Calories

Thus, the amount of heat energy required is 1031.4 Calories.

4 0

3 years ago