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Katyanochek1 [597]
2 years ago
5

In an equilibrium reaction with a Keq of 1×10^8,the-

Chemistry
1 answer:
BabaBlast [244]2 years ago
5 0
It is not exothermic because it would be negative. Since energy is required it is not spontaneous. Since heat is a reactant since the equation is endothermic since the Keq is positive, the reactants would be favored. (A)
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You use 10.0 mL of solution A, 10.0 mL of solution B, and 70.0 mL of water for your first mixture. What is the initial concentra
Katena32 [7]

Complete Question

The complete question is shown on the first uploaded image

Answer:

The  initial concentration is  C_f  =  0.0022 \  M

Explanation:

From the question we are told that

    The volume of solution A is  V_i   =  10.0 mL

    The concentration of A is C_i  =  0.0200 \ M

    The volume of solution B  is  V_B   =  10.0mL

    The volume of water is  V_{w }  =  70.0 mL

Generally the law of dilution is mathematically represented as

             C_i *  V_i = C_f *  V_f

Where  C_f is the concentration of  the mixture

            V_f is the volume of the mixture which is mathematically evaluated as

            V_f  =  10  + 10 + 70

           V_f  = 90mL

So  

      C_f  =  \frac{C_i *  V_i}{ V_f}

substituting values

       C_f  =  \frac{0.0200 *  10 }{90}

       C_f  =  0.0022 \  M

Note the mixture obtained is  KIO_3

7 0
3 years ago
Substance A is mixed with water and donates 0.4% of its H+ ions. Which of the following BEST describes Substance A? (See picture
mariarad [96]

Answer:

Explanation:

honesty i just know it has to be b or d because bases don’t donate. acids donate.

7 0
2 years ago
An object has a mass of 20 g and volume of 10 cm. Enter the numerical value for the density of the object in units of g/cmº
Nady [450]

Answer:

density = 2g/cm³

Explanation:

density = mass/volume

mass = 20g

volume = 10cm³

density = 20g/10cm³

density = 2g/cm³

6 0
3 years ago
What is the percent composition of iron in iron III chloride?
lara31 [8.8K]
The correct answer is c
7 0
2 years ago
Ammonium nitrate decomposes to dinitrogen monoxide and water. If given 45.7 grams of ammonium
statuscvo [17]

Answer:

20.54 g of H₂O

Explanation:

Since you already have a balanced equation, the next step is to see the ratio between the ammonium nitrate and water in the equation:

NH4NO3(s)—N2O(g)+2H2O

1 mole of ammonium nitrate produces 2 moles of H2O

So we have the ration:

\dfrac{1\;mole\;of\;NH_4NO_3}{2\;moles\;of\;H_{2}O}

Let's leave that for later use.

Next step is to covert the mass given into moles. We do that by getting the molar mass of the given and using that as a conversion factor:

Element   number of                 molar mass

                   atoms                  of each element          

N =                  2              x            14.01 g/mole   =      28.02 g/mole

H =                  4              x              1.01 g/mole   =        4.01  g/mole

O =                  3              x            16.00 g/mole =      <u>48.00 g/mole </u>

                                                                                    80 .03 g/mole

Now we can convert:

45.7g\;of\;NH_4NO_3\times\dfrac{1\;of\;NH_4NO_3}{80.03\;g\;of\;NH_4NO_3}=0.57\;moles\;of\;NH_4NO_3

Now we can use this to determine how many moles of H2O this would produce by using the ration we solved for earlier.

0.57\;moles\;of\;NH_4NO_3\times\dfrac{2\;moles\;of\;H_{2}O}{1\;mole\;of\;NH_4NO_3} =1.14\;moles\;of\;H_{2}O

And we convert that by getting the molecular mass of H2O, which is 18.02 g/mole:

1.14\;moles\;of\;H_{2}O\times\dfrac{18.02\;g\;of\;H_{2}O}{1\;\;mole\;of\;H_{2}O} =20.54\;g\;of\;H_{2}O

But this is only if the whole 45.7 g of ammonium nitrate is used up.

8 0
3 years ago
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