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3 years ago

What does polar and nonpolar mean in science

2 answers:

6 0

Polarity refers to the pull of electrons. Some elements like Fluorine and Oxygen pull electrons closer to them in their bonds (electronegativity), meaning they don't share them equally. So if they pull them closer, there is polarity in the molecule because there's a pull of electrons between atoms.

MissTica3 years ago

3 0

Polar molecules are molecules are essentially have no molecular symmetry.

Nonpolar molecules are molecules that have molecular symmetry.

Water is a very basic example of a polar molecule.

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Doctors have fought infections with penicillin for over 50 years. Recently, penicillin has not worked as well as before. Which o

Lilit [14]

C. "A" mentions that the drug killed all of the bacteria that are resistant to the drug, and that doesn't make any sense. "B" claims that all bacteria are resistant to the drug. This is not true. "D" mentions that bacteria eat the drug, which doesn't happen.

5 0

3 years ago

A chemist measures the amount of oxygen gas produced during an experiment. She finds that of oxygen gas is produced. Calculate t

baherus [9]

Answer:

This question is incomplete. A fragment of the question is missing. The fragment is:

She finds that 4.87 g of oxygen gas is produced

0.152 moles

Explanation:

Using the formula: mole = mass / molar mass

According to the question, a chemist measures the amount of oxygen gas produced during an experiment. Oxygen gas has the chemical formula: O2. Hence, the molar mass will be:

O2 = 16(2) = 32g/mol

If the mass of the oxygen gas to be 4.87 g of oxygen gas.

Therefore,

moles = 4.87/32

moles = 0.152mol

6 0

3 years ago

When 2.499 g of AX (s) dissolves in 135.3 g of water in a coffee-cup calorimeter the temperature rises from 23.6 °C to 35.2 °C.

Elena L [17]

Answer:

The enthalpy change for the solution process $\Delta H_{rxn}$ = - 158.34 kJ/mol

Explanation:

Given that:

The mass of salt AX = 2.499 g

The mass of water = 135.3 g

The mass of the solution = ( 2.499 + 135.3 ) g = 137.799 g

The specific heat of salt solution s is known to be = 4.18 J/g° C

The change in temperature i.e. ΔT = 35.2 °C - 23.6 °C = 11.6 °C

Thus, the amount of heat raised is equal to the heat absorbed by the calorimeter.

∴

$q_{reaction} = q_{solution}$

$q_{reaction} = -ms_{solution} \Delta T$

$q_{reaction} = -137.799 \ g \times 4.18 \dfrac{J}{g^0C}\times 11.6^0C$

$q_{reaction} = - 6682 \ J$

$q_{reaction} = - 6.682 \ kJ$

Recall that the mass of the salt = 2.499 g

The number of moles of the salt = $2.499 \ g \times \dfrac{1 \ mol \ of \ AX}{59.1097 \ g}$

= 0.0422 mol of AX

Finally the enthalpy change, $\Delta H_{rxn} = \dfrac{- 6.682 \ kJ}{ 0.0422 \ mol}$

= - 158.34 kJ/mol

The enthalpy change for the solution process $\Delta H_{rxn}$ = - 158.34 kJ/mol

3 0

3 years ago

Write the balanced chemical equation that represents the standard heat of formation of cro3(s) at 298 k.

strojnjashka [21]

The standard heat of formation is the heat released or absorbed when you obtain the CrO₃ compound. So, the reaction basically involves the individual elements of the compound. The complete balanced chemical reaction for the formation of CrO₃ is:

<em>2 Cr + 3 O₂ → 2 CrO₃</em>

6 0

3 years ago

A 0.8715 g sample of sorbic acid, a compound first obtained from the berries of a certain ash tree, is burned completely in oxyg

aivan3 [116]

<h3><u>Answer</u>;</h3>

C3H4O

<h3><u>Explanation;</u></h3>

Empirical formula is the simplest formula of a compound;

Molar mass CO2 = 44.01

Mass of CO2 produced = 2.053 g

Mass of carbon in original sample = 12.01/44.01 × 2.053

= 0.5603g

Molar mass H2O = 18

Mass of H in original sample = 2/18 ×0.5601

= 0.0622 g

Thus; original sample contained 0.5603g C and 0.0622g H. The balance of the sample was O

Mass of O = 0.8715 - (0.5603 + 0.0622) = 0.249g

The mole ratio of C:H:O will be;

Moles C = 0.5603/12 = 0.0467

Moles H = 0.0622

Moles O = 0.249/16 = 0.01556

C:H:O = 0.0467:0.0622:0.01556

Divide through by 0.01556:

C:H:O = 3:4:1

Empirical formula is thus C3H4O

8 0

4 years ago

Read 2 more answers