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3 years ago

PLEASE HELP NOW!!! 50 BRAINLEST

Chemistry

2 answers:

emmasim [6.3K]3 years ago

8 0

Answer:

It is 11 N down

Explanation:

10 N - +1 N up

Effectus [21]3 years ago

7 0

Answer:

9 N down

Explanation:

10N-1N =9 N

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Match the term to the correct definition.

nexus9112 [7]

1 is A 2 is B
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3 years ago

Read 2 more answers

Convert the following to moles.

Luda [366]

Use dimensional analysis.
$\frac{60.0 grams NaOH}{1} * \frac{1 mole NaOH}{40.0 amu NaOH} =1.5 moles$

$\frac{2.73 grams NH4Cl}{1} * \frac{1 mole NH4Cl}{53.49 amu NH4Cl} = .051 moles$

Now you try converting moles to grams. All you have to do is start with MOLES (Unlike the previous examples) over 1 then multiply that ratio by the ratio of molar mass over 1 mole. Hope this helps!

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3 years ago

The number of proton, neutrons and electrons in oxygen atom

Ksenya-84 [330]

Answer:

in an oxygen atom there are:

protons:8

electrons:8

neutrons:8

Explanation:

this is because the atomic number of oxygen is 8 and that is the proton number and the electron number is the same as the atomic number

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3 years ago

Isobutylene is a hydrocarbon used in the manufacture of synthetic rubber. when 0.847 g of isobutylene was subjected to combustio

Firlakuza [10]

Find the mass of C in the 2.657 g CO2:
(2.657 g CO2) / (44.01 g/mol) = 0.06037 mol CO2
Since each mole of CO2 also has 1 mole of C, this is equivalent to 0.06037 mol C.

Find the mass of H in the 1.089 g H2O:
(1.089 g H2O) / (18.02 g/mol) = 0.06043 mol H2O
Since 1 mol H2O has 2 mol H, this is equivalent to (0.06043)*2 = 0.1209 mol H.

Taking the ratio of H to C: 0.1209 / 0.06037 = 2.002 ~ 2
Therefore, the empirical formula of isobutylene is CH2.

6 0

3 years ago

A 0.4021-g sample of a purified organic acid was dissolved in water and titrated potentiometrically. A plot of the data revealed

Archy [21]

Answer:

The molar mass of the acid is 167.5 g/mol

Explanation:

A 0.4021-g sample of a purified organic acid was dissolved in water and titrated potentiometrically. A plot of the data revealed a single end point after 19.31 mL of 0.1243 M NaOH had been introduced. Calculate the molecular mass of the acid.

Step 1: Data given

Mass of the sample of a purified organic acid = 0.4021 grams

Molarity = 0.1243 M

Volume needed to reach the end point = 19.1 mL = 0.01931 L

Step 2: Calculate the number of moles NaOH

Moles NaOH = molarity NaOH * volume

Moles NaOH = 0.1243 M * 0.01931 L

Moles NaOH = 0.00240 moles

Step 3: Calculate moles of the acid

We'll need 0.00240 moles of acid to neutralize 0.00240 moles of NaOH ( it's a single end point)

Moles acid = 0.00240 moles

Step 4: Calculate molar mass of the acid

Molar mass = mass / moles

Molar mass = 0.4021 grams / 0.00240 moles

Molar mass = 167.5 g/mol

The molar mass of the acid is 167.5 g/mol

6 0

3 years ago