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photoshop1234 [79]
3 years ago
15

: Please predict products, label the states and write ionic and net ionic equations for each. These are all double replacement r

eactions.
please hurry
1. Magnesium hydroxide + nitic acid--
2. Potassium iodide + calcium bromide
3. Iron II bromide + silver acetate
4. Calcium hydroxide + sulfuric acid
5. Copper I bromide + lead II nitrate
6. Aluminum iodide + mercury II chloride
7. Silver nitrate + potassium phosphate
8. Ammonium chloride +mercury I acetate
9. Calcium nitrate + ammonium hydroxide
10. Copper II hydroxide + sulfurous acid
Chemistry
1 answer:
Mnenie [13.5K]3 years ago
4 0
Unmmmm i’m not quite understanding brhajsnsbfbfhrndnsnsjsmsbgbtieoou that but yes
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2 years ago
A 3.50 g sample of an unknown compound containing only C , H , and O combusts in an oxygen‑rich environment. When the products h
statuscvo [17]

Explanation:

First, calculate the moles of CO_{2} using ideal gas equation as follows.

                PV = nRT

or,          n = \frac{PV}{RT}

                = \frac{1 atm \times 4.41 ml}{0.0821 Latm/mol K \times 293 K}      (as 1 bar = 1 atm (approx))

                = 0.183 mol

As,   Density = \frac{mass}{volume}

Hence, mass of water will be as follows.

                Density = \frac{mass}{volume}

             0.998 g/ml = \frac{mass}{3.26 ml}    

                 mass = 3.25 g

Similarly, calculate the moles of water as follows.

        No. of moles = \frac{mass}{\text{molar mass}}

                              =  \frac{3.25 g}{18.02 g/mol}            

                              = 0.180 mol

Moles of hydrogen = 0.180 \times 2 = 0.36 mol

Now, mass of carbon will be as follows.

       No. of moles = \frac{mass}{\text{molar mass}}

          0.183 mol =  \frac{mass}{12 g/mol}            

                              = 2.19 g

Therefore, mass of oxygen will be as follows.

              Mass of O = mass of sample - (mass of C + mass of H)

                                = 3.50 g - (2.19 g + 0.36 g)

                                = 0.95 g

Therefore, moles of oxygen will be as follows.

          No. of moles = \frac{mass}{\text{molar mass}}

                               =  \frac{0.95 g}{16 g/mol}            

                              = 0.059 mol

Now, diving number of moles of each element of the compound by smallest no. of moles as follows.

                         C              H           O

No. of moles:  0.183        0.36       0.059

On dividing:      3.1           6.1            1

Therefore, empirical formula of the given compound is C_{3}H_{6}O.

Thus, we can conclude that empirical formula of the given compound is C_{3}H_{6}O.            

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3 years ago
The particle size of solute particles does not affects the rate. Question 14 options: True False
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