All categories

2 years ago

Directions: Determine the molar mass of the following substances.

Chemistry

1 answer:

LenaWriter [7]2 years ago

6 0

1. 40.08 + 16 = 56.08 g/mol CaO

2. 24.30 + 12.01 + 48.00 = 84.31 g/mol Mg(CO3)

3. 65.39 + 28.02 + 96 = 189.41 g/mol Zn(NO3)2

4. "Cuz" isn't an actual element. 52.00 + 64.00 = 116.00 g/mol CrO4

5. 22.99 + 1237.03 = 1260.02 g/mol Na(C103)

6. 22.99 + 32.06 = 55.05 g/mol NaS

7. 26.98 + 35.45 = 62.43 g/mol AlCl

8. 113.12 + 32.06 + 64 = 209.18 g/mol (14H4)2(SO4)

9. 176.07 + 61.94 + 128.00 = 366.01 g/mol Ni3(PO4)2

10. 137.33 + "Nn" isn't an actual element. 128.00 = 265.33 g/mol Ba(O4)2

You might be interested in

Why is vapor pressure higher in oil than water if water has stronger IMF’s?

Aleksandr-060686 [28]

Answer:

A liquid's vapor pressure is directly related to the intermolecular forces present between its molecules. The stronger these forces, the lower the rate of evaporation and the lower the vapor pressure.

Explanation:

4 0

3 years ago

Read 2 more answers

How many atoms are in 3.2 moles of chromium?

-BARSIC- [3]

Hey there!

1 mole has 6.022 x 10²³ atoms.

Multiply that by 3.2 because we have 3.2 moles.

3.2 x 6.022 x 10²³

1.9 x 10²⁴

There are 1.9 x 10²⁴ atoms in 3.2 moles of chromium.

Hope this helps!

3 0

3 years ago

. Use the following reaction to determine how much of each product would be released if 42 000 kg (42 tonnes) of methyl isocyana

fenix001 [56]

The amount of 1,3-dimethyl urea produced would be 32,458 grams or 32.458 kg while that of carbon dioxide would be 16,214 grams of 16.214 kg

<h3>Stoichiometric problem</h3>

From the equation of the reaction, the mole ratio of methyl isocyanate with the products is 2:1 respectively.

Mole of 42,000 kg of methyl isocyanate = 42000/57 = 736.84 moles

Equivalent mole of 1,3-dimethyl urea = 736.84/2 =368.42 moles

Equivaent mole of carbon dioxide = 736.84/2 =368.42moles

Mass of 368.42 moles 1,3-dimethyl urea = 368.42 x 88.1 = 32,458 grams or 32.458 kg

Mass of 368.42 moles of carbon dioxide = 368.42 x 44.01 = 16,214 grams of 16.214 kg

More on stoichiometric problems can be found here: brainly.com/question/14465605

#SPJ1

5 0

2 years ago

I NEED HELP PLEASE! :)

riadik2000 [5.3K]

Answer:

$C_{21} H_{23} NO_{5}$

Explanation:

First thing is we have assume all the percents are grams so we have

68.279g C, 6.2760g H, 3.7898g N, and 21.656g O

Now convert each gram to moles by dividing the the molar mass of each element

68.279g/12.01g= 5.685 moles of C

6.2760g/1.01g= 6.214 moles of H

3.7898g N/14.01g= 0.271 moles of N

21.656g O/ 16.00g= 1.354 moles of O

Now to find the lowest ratios divide all the moles by the smallest number of moles you found, in our case, the smallest moles is 0.271 moles of N so divide everything by that....

5.685 moles/0.271 moles ------> ~21 C

6.214 moles/0.271 moles --------> ~23 H

0.271 moles / 0.271 moles ---------> 1 N

1.354 moles/ 0.271 moles ----------> ~5 O

So the empirical formula is C21H23NO5 $C_{21} H_{23} NO_{5}$

5 0

3 years ago

If 26.2 mL of AgNO3 is needed to precipitate all the Cl− ions in a 0.785-mg sample of KCl (forming AgCl), what is the molarity o

sweet-ann [11.9K]

<u>Answer:</u>

<em>The molarity of the $AgNO_3$ solution is $4.02 \times 10^4 M$ </em>