Which is a raw material necessary for photosythisies.

The chemical formula of aspirin is C9H8O4. What is the mass of 0.40 mol<br> of aspirin?

dybincka [34]

Answer:

$\boxed {\boxed {\sf About \ 72 \ grams }}$

Explanation:

To convert from moles to grams, we must use the molar mass (also known as the gram formula mass).

First, look up the molar masses of the elements in the formula.

C: 12.011 g/mol
H: 1.008 g/mol
O: 15.999 g/mol

Next, multiply by the subscript, because it tells us the number of atoms of each element in the formula.

C₉: 4(12.011 g/mol)= 108.099 g/mol
H₈: 8(1.008 g/mol)= 8.064 g/mol
O₄: 4(15.999 g/mol)= 63.996 g/mol

Add the values.

108.099 + 8.064+63.996=180.159 g/mol

Use this molar mass as a ratio.

$\frac {180.159 \ g \ C_9H_8O_4}{1 \ mol \ C_9H_8O_4}$

Multiply by the given number of moles, 0.40

$0.40 \ mol \ C_9H_8O_4 *\frac {180.159 \ g \ C_9H_8O_4}{1 \ mol \ C_9H_8O_4}$

The units moles of aspirin cancel.

$0.40 *\frac {180.159 \ g \ C_9H_8O_4}{1 }$

$72.0636 \ g \ C_9H_8O_4$

The original number of moles has 2 sig figs (4 and 0), so answer must have the same. For the number we calculated, it is the ones place. The 0 in the tenth place tells us to leave the 2.

$72 \ g$

5 0

3 years ago

If an atom contains more <br> electrons than protons, it is

Ray Of Light [21]

Answer:

If an atom has the same number of electrons as protons, it is a neutral atom.

Explanation:

8 0

3 years ago

. Monthly measurements of atmospheric CO2 concentration at Mauna Loa began in March 1958. The average CO2 concentration for that

Harrizon [31]

Answer:

$Increase=98.8ppm$

$Average\ increase/year=1.594\frac{ppm}{year}$

Explanation:

Hello,

In this case, since the nowadays concentration of CO2 is 414.51 ppm and the concentration in 1958 was 315.71 ppm, the total increase is computed via the difference between them:

$Increase=414.51ppm-315.71ppm\\\\Increase=98.8ppm$

Moreover, the average increase per year is computed considering that from 1958 to 2020, 62 years have passed, therefore, such average is:

$Average\ increase/year=\frac{98.8ppm}{62 years} \\\\Average\ increase/year=1.594\frac{ppm}{year}$

Regards.

4 0

3 years ago

What is the empirical formula of a hydrocarbon if complete combustion or 2.900 mg of the hydrocarbon produced 9.803 mg of CO2 an

kow [346]

Answer:

The empirical formula of the hydrocarbon is CH.

Explanation:

The following data were obtained from the question:

Mass of hydrocarbon = 2.9 mg

Mass of CO2 = 9.803 mg

Mass of H2O = 2.006 mg

Next, we shall determine the mass of carbon (C) and hydrogen (H) in the compound since hydrocarbon contains carbon and hydrogen only.

This is illustrated below:

Molar mass of CO2 = 12 + (16x2) = 12 + 32 = 44 g/mol

Mass of CO2 = 9.803 mg

Mass of C in the compound =?

Mass of C in the compound =

12/44 x 9.803

= 2.674 mg

Molar mass of H2O = (2x1) + 16 = 2 + 16 = 18 g/mol

Mass of H2O = 2.006 mg

Mass of H in the compound =

2/18 x 2.006

= 0.223 mg

Finally, we shall determine the empirical formula of the hydrocarbon as follow:

Carbon (C) = 2.674 mg

Hydrogen (H) = 0.223 mg

Divide by their molar mass

C = 2.674 /12 = 0.223

H = 0.223 / 1 = 0.223

Divide both side by the the smallest

C = 0.223/0.223 = 1

H = 0.223/0.223 = 1

Therefore, the empirical formula of the hydrocarbon is CH.

5 0

3 years ago

Sue places a bucket of ice on a scale and finds that it has a mass of 3.7 kilograms. If the bucket sits for a few hours and the

butalik [34]

Hi xx can you chat for a little on snap chat

6 0

3 years ago