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Allushta [10]
3 years ago
11

1. Balance the chemical reaction for the production of hydrogen cyanide: __ NH3(g) + __ O2(g) + __ CH4(g) → __ HCN(g) + __ H2O(g

)
(Hint: none of the coefficients are larger than 6)

2.Using the balanced equation in question 1, if 25.1 g of ammonia are reacted, how many grams of hydrogen cyanide will be produced
Chemistry
1 answer:
Solnce55 [7]3 years ago
5 0
<span>2 NH</span>₃<span> + 3 O</span>₂<span> + 2 CH</span>₄<span> </span>⇒<span> 2 HCN + 6 H</span>₂<span>O
2mol                     :           2mol
34g                       :           54g
25,1g                    :           x

x = (25,1g * 54g) / 34g </span>≈ 39,9g<span>
</span>
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Which of the following will stay constant, no matter if the substance is in the solid, liquid, or gas state? volume shape temper
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Answer : The correct option is, Mass

Explanation :

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Solid state : It is a state in which the particles are closely packed and does not have any space between them. This state have a definite shape and volume.

Liquid state : It is a state in which the particles are present in random and irregular pattern. The particles are closely arranged but they can move from one place to another. This state have a definite volume but does not have a fixed shape.

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4 0
3 years ago
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7 0
2 years ago
What is the empirical formula of a compound composed of 3.25% hydrogen ( H ), 19.36% carbon ( C ), and 77.39% oxygen ( O ) by ma
Montano1993 [528]

Answer:

The answer to your question is C₂HO₃

Explanation:

Data

Hydrogen = 3.25%

Carbon = 19.36%

Oxygen = 77.39%

Process

1.- Write the percent as grams

Hydrogen = 3.25 g

Carbon = 19.36 g

Oxygen = 77.39 g

2.- Convert the grams to moles

                     1 g of H ----------------- 1 mol

                   3,25 g of H -------------  x

                     x = (3.25 x 1) / 1

                     x = 3.25 moles

                    12 g of C ---------------- 1 mol

                     19.36 g of C ----------  x

                     x = (19.36 x 1) / 12

                     x = 1.61 moles

                     16g of O --------------- 1 mol

                     77.39 g of O ---------  x

                      x = (77.39 x 1)/16

                      x = 4.83

3.- Divide by the lowest number of moles

Carbon = 3.25/1.61 = 2

Hydrogen = 1.61/1.61 = 1

Oxygen = 4.83/1.61 = 3

4.- Write the empirical formula

                        C₂HO₃

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3 years ago
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