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3 years ago

8

Isotopes that are unstable and decay when their nucleus breaks up into elements with lower atomic numbers, emitting significant

amounts of energy in the process, are called:

1 answer:

Anastaziya [24]3 years ago

5 0

Answer:

Radioactive

Explanation:

They're more unstable than my home life

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All I know is that the answer isn't c.....

gregori [183]

B. Object B is the right choice

8 0

4 years ago

A property of a substance that is the same no matter what size of sample is tested is _____.

KengaRu [80]

Answer:

B.) an intensive property

Explanation:

Bc it is a Characteristic Property that won't change no matter what size of sample is tested

6 0

3 years ago

You wish to make 250. mL of 0.20 M KCl from a stock solution of 1.5 M KCl and DI water.

Nitella [24]

The question requires us to use the dilution formula $M_iV_i=M_fV_f$ , where $M_i$ and $V_i$ are the stock concentration and volume respectively, then $M_f$ and $V_f$ are the dilute concentration and volume respectively.

a. $C_s_t_o_c_k$ = 1.5 M KCI, $C_d_i_l_u_t_e$ =0.20M KCl, $V_d_i_l_u_t_e$ =250ml KCl

b. $M_iV_i=M_fV_f\\\implies V_i= \frac{M_fV_f}{M_i} = \frac{0.20M \times 250ml}{1.5M} = 33.3\ ml$

To prepare the solution 33.3ml of 1.5M KCl is diluted to a total final volume of 250ml.

8 0

4 years ago

If salt (5. 99 × 10–6 mol) is dissolved in 1. 50 × 10–2 L of water, which expression can be used to find the molarity of the res

Alexus [3.1K]

Molarity can be defined as the moles of solute in a liter of solution. The molarity of the salt solution is $\rm \bold{3.99\;\times\;10^{-4}\;M}$ .

<h3>What is the relation between moles and volume?</h3>

The moles are the mass of substance with respect to the molar mass. The moles and volume relationship can be expressed in terms of molarity.

The molarity can be expressed as:

$\rm Molarity=\dfrac{Moles}{Volume}$

The given solution has,

Moles of salt = $\rm 5. 99\;\times\; 10^-^6$

The volume of solution = $\rm 1.50\;\times\;10^-^2$ L.

Substituting the values for molarity as:

$\rm Molarity=\dfrac{5.99\;\times\;10^{-6}}{1.50\;\times\;10^-^2\;L}\\ Molarity=3.99\;\times\;10^{-4}\;M$

The molarity of the solution is $\rm \bold{3.99\;\times\;10^{-4}\;M}$ . Thus, option C is correct.

Learn more about molarity, here:

brainly.com/question/12127540

4 0

3 years ago

Given that it requires 27.9 ml of 0.270 m na2s2o3(aq) to titrate a 15.0-ml sample of i3–(aq), calculate the molarity of i3–(aq)

Digiron [165]

The molar concentration of the KI_3 solution is 0.251 mol/L.

<em>Step 1</em>. Write the <em>balanced chemical equation</em>

I_3^(-) + 2S_2O_3^(2-) → 3I^(-) + S_4O_6^(2-)

<em>Step 2</em>. Calculate the <em>moles of S_2O_3^(2-)</em>

Moles of S_2O_3^(2-)

= 27.9 mL S_2O_3^(2-) ×[0.270 mmol S_2O_3^(2-)/(1 mL S_2O_3^(2-)]

= 7.533 mmol S_2O_3^(2-)

<em>Step 3</em>. Calculate the <em>moles of I_3^(-) </em>

Moles of I_3^(-) = 7.533 mmol S_2O_3^(2-)))) × [1 mmol I_3^(-)/(2 mmol S_2O_3^(2-)] = 3.766 mmol I_3^(-)

<em>Step 4</em>. Calculate the <em>molar concentration of the I_3^(-) </em>

<em>c</em> = "moles"/"litres" = 3.766 mmol/15.0 mL = 0.251 mol/L

6 0

4 years ago