What happens when a atom losses 2 electrons

The table shows the specific heat of four substances—brick, dry soil, paper, and water. If all four substances were exposed to s

Anvisha [2.4K]

The specific heat is the amount of heat per unit mass required to raise the temperature by one degree Celsius. Therefore, a high value of specific heat would mean that more heat is needed in order for the temperature to increase. The correct answer would be water since it has the highest specific heat of the choices given.

7 0

2 years ago

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To what class of minerals do gold, silver, and copper belong? A. carbonates B. native elements C. halides D. sulfates and sulfid

Nataly_w [17]

I have never heard of the term native elements before but that must be it since carbonates contain CO₃, halides contain a halogen, and sulfates and sulfide contain either SO₄ or SO₃. Gold, silver, and copper can all become carbonates, sulfates or sulfides, and halides. However, by them selves they don't.

4 0

3 years ago

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How many grams are there in 1.5x10^25 molecules of CO2?

Arturiano [62]

Answer:

Now, a substance's molar mass tells what the mass of one mole of that substance is. In carbon dioxide's case, its molar mass is equal to 44.01 g/mol , which means that every mole of CO2 will have a mass of 44.01 g

Explanation:

5 0

2 years ago

Which of the following terms measures the amount of matter in an object? Weight or mass

Oksanka [162]

Mass measures the amount of matter in an object

3 0

2 years ago

Suppose 0.245 g of sodium chloride is dissolved in 50. mL of a 18.0 m M aqueous solution of silver nitrate.

Bezzdna [24]

Answer:

$\large \boxed{\text{ 0.066 mol/L}}$

Explanation:

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

1. Assemble all the data in one place, with molar masses above the formulas and other information below them.

Mᵣ: 58.44

NaCl + AgNO₃ ⟶ NaNO₃ + AgCl

m/g: 0.245

V/mL: 50.

c/mmol·mL⁻¹: 0.0180

2. Calculate the moles of each reactant

$\text{Moles of NaCl} = \text{245 mg NaCl} \times \dfrac{\text{1 mmol NaCl}}{\text{58.44 mg NaCl}} = \text{4.192 mmol NaCl}\\\\\text{ Moles of AgNO}_{3}= \text{50. mL AgNO}_{3} \times \dfrac{\text{0.0180 mmol AgNO}_{3}}{\text{1 mL AgNO}_{3}} = \text{0.900 mmol AgNO}_{3}$

3. Identify the limiting reactant

Calculate the moles of AgCl we can obtain from each reactant.

From NaCl:

The molar ratio of NaCl to AgCl is 1:1.

$\text{Moles of AgCl} = \text{4.192 mmol NaCl} \times \dfrac{\text{1 mmol AgCl}}{\text{1 mmol NaCl}} = \text{4.192 mmol AgCl}$

From AgNO₃:

The molar ratio of AgNO₃ to AgCl is 1:1.

$\text{Moles of AgCl} = \text{0.900 mmol AgNO}_{3} \times \dfrac{\text{1 mmol AgCl}}{\text{1 mmol AgNO}_{3}} = \text{0.900 mmol AgCl}$

AgNO₃ is the limiting reactant because it gives the smaller amount of AgCl.

4. Calculate the moles of excess reactant

Ag⁺(aq) + Cl⁻(aq) ⟶ AgCl(s)

I/mmol: 0.900 4.192 0

C/mmol: -0.900 -0.900 +0.900

E/mmol: 0 3.292 0.900

So, we end up with 50. mL of a solution containing 3.292 mmol of Cl⁻.

5. Calculate the concentration of Cl⁻

$\text{[Cl$^{-}$] } = \dfrac{\text{3.292 mmol}}{\text{50. mL}} = \textbf{0.066 mol/L}\\\text{The concentration of chloride ion is $\large \boxed{\textbf{0.066 mol/L}}$}$

8 0

2 years ago