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netineya [11]
2 years ago
13

? + ? = zink chloride + water​

Chemistry
1 answer:
Elodia [21]2 years ago
8 0

Answer:

Zinc, hydrochloric acid

Explanation:

A metal plus an acid equals a salt plus water

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The "particles" of gases are actually atoms, or molecules. truefalse
kirill [66]
They are atoms. a molecule is made up of atoms. 
8 0
3 years ago
When a mixture of 12.0 g of acetylene (c2h2 and 12.0 g of oxygen (o2 is ignited, the resultant combustion reaction produces co2
valina [46]
The product of the complete combustion of any fuel (in this case, acetylene) are indeed water and carbon dioxide. 
Balancing the combustion reaction,
                           C2H2 +(5/2) O2 --> 2CO2 + H2O
The number of moles of C2H2 will be,
                        (12 g) x (1 mole/26 g) = 6/13 mole
Then, the number of moles of O2 is,
                         (12 g) x (1 mole/32 g) = 3/8 mole
Therefore the limiting reaction is the O2. Getting the amount of CO2 and H2O produced from balancing,
             CO2 = (3/8 moles) x (2 moles CO2/ 5/2 mole O2)(44 g/ 1 mole) = 52.8 g
             H2O = (3/8 moles) x (1 mole / 5/2 mole O2)(18 g / 1 mole) = 2.7 g
3 0
3 years ago
Read 2 more answers
During photosynthesis, light energy from the Sun causes a reaction to take place. The products of photosynthesis are used in a r
andrew11 [14]

Answer:

chemical reactions which proceed with the release of heat energy are called exothermic reactions

3 0
2 years ago
12.47 g of ammonium nitrate are dissolved in water, then diluted to 250 ml. What is the molarity of the resulting solution?
slega [8]
<h3><u>Answer;</u></h3>

= 0.6224 M

<h3><u>Explanation</u>;</h3>

Molarity is given by the formula;

Molarity = Number of moles/Volume

But moles = mass/Molar mass

Thus;

Moles = 12.47 g/80.043 g/mol

          = 0.1556 Moles

Therefore;

Molarity = 0.1556 moles/0.25

<h3>            <u>= 0.6224 M</u></h3>

6 0
3 years ago
Pyridinium is a weak acid having a pKa of 5.2. How much pyridine (the conjugate base of pyridinium) must be added to an aqueous
Whitepunk [10]

Answer:

Amount of pyridine required = 0.0316 M

Explanation:

pH of a buffer solution is calculated by using Henderson - Hasselbalch equation.

pH=pK_a+log\frac{[Conjugate\ base]}{[weak\ acid]}

Pyridinium is a weak acid and in the presence of its conjugate base, it acts as buffer.

Henderson - Hasselbalch equation for pyridine/pyridinium buffer is as follows:

pH=pK_a+log\frac{[Py]}{PyH^+]}

pH = 4.7

pK_a=5.2

PyH^+ (Pyridinium)=0.100 M

Substitute the values in the formula

pH=pK_a+log\frac{[Py]}{PyH^+]}\\4.7=5.2 log\frac{[Py]}{0.100}

4.7-5.2=log\frac{[Py]}{0.100} \\-0.5=log\frac{[Py]}{0.100}\\\frac{[Py]}{0.100}=antilog -0.5\\\frac{[Py]}{0.100}=0.316

\frac{[Py]}{0.100} =0.316

[Py]=0.0316\ M

Amount of pyridine required = 0.0316 M

7 0
2 years ago
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