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IgorLugansk [536]
3 years ago
9

Enter the net ionic equation, including phases, for the reaction of AgNO3(aq) with K2SO4(aq). Solubility Rules are found here.

Chemistry
1 answer:
Inessa05 [86]3 years ago
5 0
Write out the equation: 
AgNO3(aq)+K2SO4(aq) --> Ag2SO4(s)+K2(NO3)... 

Balance the equation: 
2 AgNO3(aq)+K2SO4(aq) --> Ag2SO4(s)+K2(NO3)2... 

Remember to keep molecules intact when you write out the ions.
(2Ag+)+(2NO3-)+(2K+)+(SO42-) --> (Ag2SO42
Cancel out all the spectator ions. These are ions that watch the reaction that didn't change. For this problem 2K+ & 2NO3- are the spectator ions. 

You are left with your net ionic equation of
2Ag+(aq)+SO42-(aq)-->Ag2SO4(s)
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What is the mass of 2.40 moles of magnesium chloride, mgcl2
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Hey there!

MgCl₂

Find molar mass of magnesium chloride.

Mg: 1 x 24.305

Cl: 2 x 35.453

--------------------  

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One mole of magnesium chloride has a mass of 95.211 grams.

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2.40 x 95.211 = 228.5

To 3 sig figs this is 229.

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Hope this helps!

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3 years ago
In a mixture of hydrogen and nitrogen gases, the mole fraction of nitrogen is 0.333. If the partial pressure of hydrogen in the
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Answer:

P_T=112.4torr

Explanation:

Hello there!

In this case, since these problems about gas mixtures are based off Dalton's law in terms of mole fraction, partial pressure and total pressure, we can write the following for hydrogen, we are given its partial pressure:

P_{H_2}=x_{H_2}*P_T

And can be solved for the total pressure as follows:

P_T=\frac{P_{H_2}}{x_{H_2}}

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Regards!

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