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sladkih [1.3K]
3 years ago
9

*click image*

Chemistry
1 answer:
nadya68 [22]3 years ago
6 0

Answer:

Its be 1,2 and 4.

Explanation:

Since changing the direction won't do anything to a electric magnet.

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If he(g) has an average kinetic energy of 8750 j/mol under certain conditions, what is the root mean square speed of cl2(g) mole
saw5 [17]
<span>The root mean square speed is given by V_rms = âšRT/M where r, t, and m are the rate constant, temperature and molar mass the gas Average molar kinetic energy of the gas E = 1/2 M * (V_rms)^2 = 8750 ms/1 So (V_rms)^2 = (2 * 8750) / M Molar mass of 2 chlorine atoms in kg is 2 * 35 * 10^(-3) Hence we have (V_rms)^2 = (2 * 8750)/ (2 * 35 * 10^(-3)) (V_rms)^2 = 8750/0.035 = 250000 So V_rms = âš 250000 = 500</span>
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3 years ago
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Yeast cells thrive on ice cold water *<br> True<br> оо<br> False
NemiM [27]

Answer:

TRUE

Explanation:

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2 years ago
Which phase change in an example of an exothermic process?
photoshop1234 [79]
C. liquid to solid  i hope this helps

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3 years ago
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A compound contains 6.0 g of carbon and 1.0 g of hydrogen and has a molar mass of 42.0 g/mol.
makvit [3.9K]

Answer:

%C = 85.71 wt%; %H = 14.29 wt%; Empirical Formula => CH₂; Molecular Formula => C₃H₆

Explanation:

%Composition

Wt C = 6 g

Wt H = 1 g

TTL Wt = 6g + 1g = 7g

%C per 100wt = (6/7)100% = 85.71 wt%

%H per 100wt = (1/7)100% = 14.29 wt % or, %H = 100% - %C = 100% - 85.71% = 14.29 wt% H

What you should know when working empirical formula and molecular formula problems.

Empirical Formula=> <u>smallest</u> whole number ratio of elements in a compound

Molecular Formula => <u>actual</u> whole number ratio of elements in a compound

Empirical Formula Weight x Whole Number Multiple = Molecular Weight

From elemental %composition values given (or, determined as above), the empirical formula type problem follows a very repeatable pattern. This is ...

% => grams => moles => ratio => reduce ratio => empirical ratio

for determination of molecular formula one uses the empirical weight - molecular weight relationship above to determine the whole number multiple for the molecular ratios.

Caution => In some 'textbook' empirical formula problems, the empirical ratio may contain a fraction in the amount of 0.25, 0.50 or 0.75. If such an issue arises, multiply all empirical ratio numbers containing 0.25 and/or 0.75 by '4'  to get the empirical ratio and multiply all empirical ration numbers containing 0.50 by '2' to get the final empirical ratio.

This problem:

Empirical Formula:

Using the % per 100wt values in part 'a' ...

              %     =>         grams                 =>                 moles

%C => 85.71% => 85.71 g* / 100 g Cpd => (85.71 / 12) = 7.14 mol C

%H => 14.29% => 14.29 g / 100 g Cpd => (14.29 / 1) = 14.29 mol H

=> Set up mole Ratio and Reduce to Empirical Ratio:

mole ratio C:H =>  7.14 : 14.29

<u>To reduce mole values to the smallest whole number ratio,  divide all mole values by the smaller mole value of the set.</u>

=> 7.14/7.14 : 14.29/7.14 => Empirical Ration=> 1 : 2

∴ Empirical Formula => CH₂

Molecular Formula:

(Empirical Formula Wt)·N = Molecular Wt => N = Molecular Wt / Empirical Wt

N = 42 / 14 = 3 => multiply subscripts of empirical formula by '3'.

Therefore, the molecular formula is C₃H₆

3 0
3 years ago
The table shows the volumes of different samples of liquid? Which sample has the greatest DENSITY.
arlik [135]

Answer:

Maybe B

Explanation:

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