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Anna007 [38]
3 years ago
10

All of the following conditions of STP are true except A. 101.3 kPa B. 273.15 K C. 22.4 L D. 3.81 kPa

Chemistry
1 answer:
kaheart [24]3 years ago
8 0
  3.81   kpa  is  the  condition   which  is  not  true   at  STP

According  to  IUPAC  the  standard  temperature  and  pressure  that  is  STP  the  temperature  is   273.15  k  or  0   degrees  celsius .  and  the  absolute  temperature   of   101.325 Kpa   or  1  atm.  In  addition at STP   the  volume of  ideal  gas  is  22.4 
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Formula of sodium carbonate​
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Working on-board a research vessel somewhere at sea, you have (carefully) isolated 12.5 micrograms (12.5 ×10–6 g) of what you ho
german

Answer:

The value is Z  =  311.33 \ g/mol

Explanation:

From the question we are told that

The mass of saxitoxin is m  =  12.5 mg = 12.5 * 10^{-6} g

The volume of water is V  =  3.10  mL  =  3.10 *10^{-3} L

The osmotic pressure is P =  0.236 =  \frac{0.236}{760}  =  3.105 * 10^{-4} atm

The temperature is T  =  19^oC  =  19 + 273 =  292 \  K

Generally the osmotic pressure is mathematically represented as

P  =  C  *  T  * R

Here R is the gas constant with value

R =  0.0821 ( L .atm /mol. K)

and C is the concentration of saxitoxin

So

3.105 * 10^{-4}  =  C * 0.0821   *  292

C = 1.295 *10^{-5} mol/L

Generally the number of moles of saxitoxin is mathematically represented as

n = C  *  V

=> n = 1.295 *10^{-5}   *3.10 *10^{-3}

=> n = 4.015 *10^{-8} \  mol

Generally the molar mass of saxitoxin is mathematically represented as

Z  =  \frac{m}{n}

=> Z  =  \frac{12.5 * 10^{-6}}{ 4.015 *10^{-8}}

=> Z  =  311.33 \ g/mol

5 0
3 years ago
Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure. Identify the limiting r
djyliett [7]

Answer:

* Limiting reagent: potassium.

* m_{Cl_2}^{excess}=2.47gCl_2

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

2K(s)+Cl_2(g)\rightarrow 2KCl

In such a way, the reacting moles of chlorine are:

n_{Cl_2}=7.00g*\frac{1molCl_2}{70.9gCl_2}=0.0987molCl_2

Now, the amount of chlorine gas that would react with 5.00 g of potassium result:

n_{Cl_2}^{consumed}=5.00g*\frac{1molK}{39.1gK}*\frac{1molCl_2}{2molK}=0.0639molCl_2

Thus, the chlorine will be in excess and the potassium will be the limiting reagent. Therefore, the mass of excess chlorine turns out:

m_{Cl_2}^{excess}=(0.0987-0.0639)molCl_2*\frac{70.9gCl_2}{1molCl_2}=2.47gCl_2

Best regards.

4 0
3 years ago
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