Look at the picture of the fragmented rock.

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (c2h6o2) dissolved in 500.0 g of water. kf = 1.86Â°c/m a

Bingel [31]

Answer:The boiling point of the solution is 108° C.

Explanation:

Boiling point of pure water=T= $100^oC$

Boiling point of water after addition of 500 g of ethylene glycol= $T_f$

Mass of water = 500g = 0.5 kg (1000 g = 1 kg)

$\Delta T_f=K_b\times \frac{\text{Mass of ethlyene glycol}}{\text{Molar mass of ethylene glycol}}$

$\Delta T_f=0.512^oC/m\times \frac{500 g}{62.07 g/mol\times 0.5 kg}$

$\Delta T_f=8.24 ^oC$

$\Delta T_f=T_f-T$

$8.24^oC=T_f-100^oC$

$T_f=108.24^oC$

The boiling point of the solution is 108° C.

7 0

3 years ago

Silver sulfadiazine burn-treating cream creates a barrier against bacterial invasion and releases antimicrobial agents directly

trapecia [35]

Answer : The mass of silver sulfadiazine produced can be, 71.35 grams.

Solution : Given,

Mass of $Ag_2O$ = 25.0 g

Mass of $C_{10}H_{10}N_4SO_2$ = 50.0 g

Molar mass of $Ag_2O$ = 231.7 g/mole

Molar mass of $C_{10}H_{10}N_4SO_2$ = 250.3 g/mole

Molar mass of $AgC_{10}H_{9}N_4SO_2$ = 357.1 g/mole

First we have to calculate the moles of $Ag_2O$ and $C_{10}H_{10}N_4SO_2$ .

$\text{ Moles of }Ag_2O=\frac{\text{ Mass of }Ag_2O}{\text{ Molar mass of }Ag_2O}=\frac{25.0g}{231.7g/mole}=0.1079moles$

$\text{ Moles of }C_{10}H_{10}N_4SO_2=\frac{\text{ Mass of }C_{10}H_{10}N_4SO_2}{\text{ Molar mass of }C_{10}H_{10}N_4SO_2}=\frac{50.0g}{250.3g/mole}=0.1998moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$Ag_2O(s)+2C_{10}H_{10}N_4SO_2(s)\rightarrow 2AgC_{10}H_9N_4SO_2(s)+H_2O(l)$

From the balanced reaction we conclude that

As, 2 mole of $C_{10}H_{10}N_4SO_2$ react with 1 mole of $Ag_2O$

So, 0.1998 moles of $C_{10}H_{10}N_4SO_2$ react with $\frac{0.1998}{2}=0.0999$ moles of $Ag_2O$

From this we conclude that, $Ag_2O$ is an excess reagent because the given moles are greater than the required moles and $C_{10}H_{10}N_4SO_2$ is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of $AgC_{10}H_9N_4SO_2$

From the reaction, we conclude that

As, 2 mole of $C_{10}H_{10}N_4SO_2$ react with 2 mole of $AgC_{10}H_9N_4SO_2$

So, 0.1998 mole of $C_{10}H_{10}N_4SO_2$ react with 0.1998 mole of $AgC_{10}H_9N_4SO_2$

Now we have to calculate the mass of $AgC_{10}H_9N_4SO_2$

$\text{ Mass of }AgC_{10}H_9N_4SO_2=\text{ Moles of }AgC_{10}H_9N_4SO_2\times \text{ Molar mass of }AgC_{10}H_9N_4SO_2$

$\text{ Mass of }AgC_{10}H_9N_4SO_2=(0.1998moles)\times (357.1g/mole)=71.35g$

Therefore, the mass of silver sulfadiazine produced can be, 71.35 grams.

8 0

3 years ago

A student titrates a solution containing 0.050 moles of calcium hydroxide with phosphoric acid. How many moles of phosphoric aci

lina2011 [118]

Answer:

The answer to your question is 0.33 moles of H₃PO₄

Explanation:

Data

moles of Ca(OH)₂ = 0.050

moles of H₃PO₄ = ?

Process

1.- Write the balanced chemical equation

3Ca(OH)₂ + 2H₃PO₄ ⇒ Ca₃(PO₄)₂ + 6H₂O

Reactants Elements Products

3 Ca 3

12 H 12

14 O 14

2.- Calculate the moles of phosphoric acid

3 moles of calcium hydroxide --------------- 2 moles of phosphoric acid

0.5 moles of calcium hydroxide ----------- x

x = (0.5 x 2)/3

x = 0.33 moles

6 0

3 years ago

Which hydrogen is an unsaturated hydrocarbon ?

Ksivusya [100]

Answer:

Image result for Which hydrogen is an unsaturated hydrocarbon ?

Alkenes have the general formula CnH2n, and are examples of unsaturated hydrocarbons. The presence of a double bond compound's structure causes there to be two fewer hydrogen atoms in the molecule than there are in an alkane with the same number of carbon atoms.

3 0

3 years ago

What type of rock would you expect to form as the result of an explosive eruption?

Vedmedyk [2.9K]

The correct answer is Pumice.

4 0

3 years ago

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