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Arturiano [62]
2 years ago
5

your mother, who is a self-described chocolate addict, phones you. she has read in the newspaper a summary of a research study s

uggesting that the consumption of a moderate amount of bittersweet chocolate reduces the risk of heart disease in older women. you ask her who funded the research. She says doesn't know and asks you why it would matter.
Chemistry
1 answer:
son4ous [18]2 years ago
7 0

Answer:

This matters because you need to know if this site is crediable

Explanation:

You need to know this because you need to know who runs this site and if it was approved by anything crediable.

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1. A student collected the following data for a fixed volume of gas: Temperature (⁰C) Pressure (mm of Hg) 10 726 20 750 40 800 7
zimovet [89]

Answer is: the missing pressure is 1088.66 mmHg.

Gay-Lussac's Law states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature.

p₁/T₁ = p₂/T₂.

p₁ = 960 mmHg; pressure of the gas.

T₁ = 100°C + 273.15.

T₁ = 373.15 K; temperature of the gas.

T₂ = 150°C + 273.15.

T₂ = 423.15 K.

p₂ = p₁T₂/T₁.

p₂ = 960 mmHg · 423.15 K / 373.15 K.

p₂ = 1088.66 mmHg.

6 0
3 years ago
When solutions of magnesium chloride and potassium phosphate are combined write the formula for the precipitate formed
Zielflug [23.3K]
The products will be magnesium phosphate and potassium chloride. You then have to watch a solubility chart to see which one of these is not soluable. In this case it is magnesium phosphate.
6 0
3 years ago
Empirical formula of a compound composed of 32.1 g potassium (k) and 6.57 g oxygen (o)?
tester [92]

The empirical formula is K₂O.

The empirical formula is the <em>simplest whole-number ratio</em> of atoms in a compound.

The <em>ratio of atom</em>s is the same as the <em>ratio of moles</em>.

So, our job is to calculate the <em>molar ratio</em> of K to O.

Step 1. Calculate the <em>moles of each element </em>

Moles of K = 32.1 g K × (1 mol K/(39.10 g K =) = 0.8210 mol K

Moles of O = 6.57 g O × (1 mol O/16.00 g O) = 0.4106 mol 0

Step 2. Calculate the <em>molar ratio of each elemen</em>t

Divide each number by the smallest number of moles and round off to an integer

K:O = 0.8210:0.4106 = 1.999:1 ≈ 2:1

Step 3: Write the <em>empirical formula </em>

EF = K₂O

5 0
3 years ago
The following molecular equation represents the reaction that occurs when aqueous solutions of silver(I) nitrate and calcium chl
dsp73

Answer:

Ag+(aq) + Cl-(aq) —> AgCl(s)

Explanation:

2AgNO3(aq) + CaCl2(aq) —>2AgCl(s) + Ca(NO3)2(aq)

The balanced net ionic equation for the reaction above can be obtained as follow:

AgNO3(aq) and CaCl2(aq) will dissociate in solution as follow:

AgNO3(aq) —> Ag+(aq) + NO3-(aq)

CaCl2(aq) —> Ca2+(aq) + 2Cl-(aq)

AgNO3(aq) + CaCl2(aq) –>

2Ag+(aq) + 2NO3-(aq) + Ca2+(aq) + 2Cl-(aq) —> 2AgCl(s) + Ca2+(aq) + 2NO3-(aq)

Cancel out the spectator ions i.e Ca2+(aq) and 2NO3- to obtain the net ionic equation.

2Ag+(aq) + 2Cl-(aq) —> 2AgCl(s)

Divide through by 2

Ag+(aq) + Cl-(aq) —> AgCl(s)

The, the net ionic equation is

Ag+(aq) + Cl-(aq) —> AgCl(s)

4 0
3 years ago
Solid sodium metal reacts violently with water, producing heat, hydrogen gas, and sodium hydroxide. How many molecules of hydrog
asambeis [7]

Answer:

4.6 × 10²³ molecules:

Step-by-step solution

You will need a balanced equation with masses, moles, and molar masses, so let's gather the information in one place:

M_r:  22.99

          2Na + 2H₂O ⟶ 2NaOH + H₂

m/g:    35

1. Calculate the <em>moles of Na </em>

Moles of Na = 35 g Na × (1 mol Na/22.99 g Na)

Moles of Na = 1.52 mol Na

2. Calculate the <em>moles of H₂ </em>

Moles of H₂ = 1.52 mol Na × (1 mol H₂/2 mol Na)

Moles of H₂= 0.761 mol H₂

3. Calculate the molecules of H₂

6.022 × 10²³ molecules H₂ = 1 mol H₂

                Molecules of H₂ = 0.761 × (6.022 × 10²³ /1)

                Molecules of H₂ = 4.6 × 10²³ molecules H₂

The reaction forms 4.6 × 10²³ molecules of H₂.

5 0
3 years ago
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