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77julia77 [94]
2 years ago
10

What volume of 1.25 M sodium hydroxide (NaOH) solution can be prepared using 60.0 g of sodium hydroxide? (The mass of one mole o

f NaOH is 40.0 g.)
0.667 L
0.833 L
1.20 L
1.88L
Chemistry
1 answer:
nataly862011 [7]2 years ago
8 0

Answer:

The answer is

<h2>1.20 L</h2>

Explanation:

Since the concentration , mass and molar mass of NaOH has been given we use the formula

<h3>C =  \frac{m}{M \times v}</h3>

To find the volume

where

C is the concentration

m is the mass

M is the molar mass

v is the volume

Making volume the subject we have

<h3>v =  \frac{m}{C \times M}</h3>

From the question

C = 1.25 M

m = 60 g

M = 40.0 g/mol

Substitute the values into the above formula and solve for the volume

We have

<h3>v =  \frac{60}{1.25 \times 40}  \\ v =  \frac{60}{50}  \\ v =  \frac{6}{5}</h3>

We have the final answer as

<h3>Volume = 1.20 L</h3>

Hope this helps you

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Calculate the initial rate for the formation of C at 25 ∘C, if [A]=0.50M and [B]=0.075M.Express your answer to two significant f
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The question is incomplete, here is the complete question:

Calculate the initial rate for the formation of C at 25°C, if [A]=0.50 M and [B]=0.075 M. Express your answer to two significant figures and include the appropriate units.Consider the reaction

A + 2B ⇔ C

whose rate at 25°C was measured using three different sets of initial concentrations as listed in the following table:

The table is attached below as an image.

<u>Answer:</u> The initial rate for the formation of C at 25°C is 2.25\times 10^{-2}Ms^{-1}

<u>Explanation:</u>

Rate law is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

For the given chemical equation:

A+2B\rightleftharpoons C

Rate law expression for the reaction:

\text{Rate}=k[A]^a[B]^b

where,

a = order with respect to A

b = order with respect to B

  • Expression for rate law for first trial:

5.4\times 10^{-3}=k(0.30)^a(0.050)^b ....(1)

  • Expression for rate law for second trial:

1.1\times 10^{-2}=k(0.30)^a(0.100)^b ....(2)

  • Expression for rate law for third trial:

2.2\times 10^{-2}=k(0.50)^a(0.050)^b ....(3)

Dividing 2 by 1, we get:

\frac{1.1\times 10^{-2}}{5.4\times 10^{-3}}=\frac{(0.30)^a(1.00)^b}{(0.30)^a(0.050)^b}\\\\2=2^b\\b=1

Dividing 3 by 1, we get:

\frac{2.2\times 10^{-2}}{5.4\times 10^{-3}}=\frac{(0.50)^a(0.050)^b}{(0.30)^a(0.050)^b}\\\\4.07=2^a\\a=2

Thus, the rate law becomes:

\text{Rate}=k[A]^2[B]^1       ......(4)

Now, calculating the value of 'k' by using any expression.

Putting values in equation 1, we get:

5.4\times 10^{-3}=k[0.30]^2[0.050]^1\\\\k=1.2M^{-2}s^{-1}

Calculating the initial rate of formation of C by using equation 4, we get:

k=1.2M^{-2}s^{-1}

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[B] = 0.075 M

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\text{Rate}=1.2\times (0.50)^2\times (0.075)^1\\\\\text{Rate}=2.25\times 10^{-2}Ms^{-1}

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