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AleksandrR [38]
3 years ago
5

Calculate the density of a rock if it has a mass of 498g and a volume of 11.9 mL.

Chemistry
1 answer:
Free_Kalibri [48]3 years ago
5 0

Answer:

<h2>Density = 41.8 g/mL</h2>

Explanation:

The density of a substance can be found by using the formula

<h3>Density =  \frac{mass}{volume}</h3>

From the question

mass = 498 g

volume = 11.9 mL

Substitute the values into the above formula and solve for the Density

That's

<h3>Density =  \frac{498}{11.9}  \\   = 41.8487</h3>

We have the final answer as

<h3>Density = 41.8 g/mL</h3>

Hope this helps you

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To plot the calibration curve, you need to prepare iron solutions with known concentrations and measure their absorbance.
kap26 [50]

To plot the calibration curve, you need to prepare iron solutions with known concentrations and measure their absorbance. You need to pipet 0 mL of the diluted solution to have 0.00 mg of iron.

In spectrophotometry, to plot the calibration curve, you need to prepare solutions with known concentrations and measure their absorbance.

We have a standard iron solution with a concentration of 0.2500g/L of pure iron (C₁). We pipet 25.00mL (V₁) of this standard iron solution into a 500mL (V₂) volumetric flask and dilute up to the mark with distilled water.

We can calculate the concentration of the diluted solution (C₂) using the dilution rule.

C_1 \times V_1 = C_2 \times V_2\\\\C_2 = \frac{C_1 \times V_1}{V_2}  = \frac{0.2500 g/L \times 25.00 mL}{500 mL} = 0.0125 g/L

Then, if we wanted to prepare the blank, that is, the solution that contains the same matrix but not the analyte, and whose concentration in iron is 0.00 mg/L, we wouldn't pipet any of the diluted solution.

To plot the calibration curve, you need to prepare iron solutions with known concentrations and measure their absorbance. You need to pipet 0 mL of the diluted solution to have 0.00 mg of iron.

Learn  more: brainly.com/question/24195565

8 0
2 years ago
6. The graph below shows the heating curve for ethanol (from –200C to 150C). Calculate the amount of heat (kJ) required for each
Kazeer [188]

This problem is providing the heating curve of ethanol showing relevant data such as the initial and final temperature, melting and boiling points, enthalpies of fusion and vaporization and specific heat of solid, liquid and gaseous ethanol, so that the overall heat is required and found to be 1.758 kJ according to:

<h3>Heating curves:</h3>

In chemistry, we widely use heating curves in order to figure out the required heat to take a substance from a temperature to another. This process may involve sensible heat and latent heat, when increasing or decreasing the temperature and changing the phase, respectively.

Thus, since ethanol starts off solid and end up being a vapor, we will find five types of heat, three of them related to the heating-up of ethanol, firstly solid, next liquid and then vapor, and the other two to its fusion and vaporization as shown below:

Q_T=Q_1+Q_2+Q_3+Q_4+Q_5

Hence, we begin by calculating each heat as follows, considering 1 g of ethanol is equivalent to 0.0217 mol:

Q_1=0.0217mol*111.5\frac{J}{mol*\°C}[(-114.1\°C)-(-200\°C)] *\frac{1kJ}{1000J} =0.208kJ\\&#10;\\&#10;Q_2=0.0217mol*4.9\frac{kJ}{mol} =0.106kJ\\&#10;\\&#10;Q_3=0.0217mol*112.4\frac{J}{mol*\°C}[(78.4\°C)-(-114.1\°C)] *\frac{1kJ}{1000J} =0.470kJ\\&#10;\\&#10;Q_4=0.0217mol*38.6\frac{kJ}{mol} =0.838kJ\\&#10;\\&#10;Q_5=0.0217mol*87.5\frac{J}{mol*\°C}[(150\°C)-(78.4\°C)] *\frac{1kJ}{1000J} =0.136kJ

Finally, we add them up to get the result:

Q_T=0.208kJ+0.106kJ+0.470kJ+0.838kJ+0.136kJ\\&#10;\\&#10;Q_T=1.758kJ

Learn more about heating curves: brainly.com/question/10481356

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