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Marta_Voda [28]
3 years ago
5

What are the 6 types of chemical reactions?

Chemistry
2 answers:
marusya05 [52]3 years ago
6 0

Answer:

Combination.

Decomposition.

Single displacement.

Double displacement.

Combustion.

Redox.

Nadusha1986 [10]3 years ago
4 0

Answer:

Explanation:

Six common types of chemical reactions are: synthesis, decomposition, single-displacement, double-displacement, combustion and acid-base reactions .

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2 years ago
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A 25.00 ml sample of h3po4 solution is neutralized by exactly 54.93 ml of 0.04345 m ca(oh)2. what is the molarity of the h3po4 s
son4ous [18]
The neutralization equation is:
3 Ca(OH)₂ + 2 H₃PO₄ → Ca₃(PO₄)₂ + 6 H₂O

From this equation we can see that 3 moles of Ca(OH)₂ react with 2 moles of H₃PO₄

Numbers of mmol of Ca(OH)₂ = M x V = 0.04345 x 54.93 = 2.387 mmol

Number of mmol of H₃PO₄ = 2.387 x (2/3) = 1.591 mmol

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8 0
3 years ago
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Use the Lewis model to determine the formula for the compound that forms from each pair of atoms.
Oksi-84 [34.3K]

Answer:

KI

Explanation:

K is 1+  & I is 1- so we need 1 of each to balance out the compound.

8 0
3 years ago
If it takes 38.70cm of 1.90M NaOH to neutralize 10.30cm of H2SO4 in a battery, what is the molarity of H2SO4?
slamgirl [31]

Answer:

The molarity of the acid, H₂SO₄ is 3.57 M

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

H₂SO₄ + 2NaOH —> Na₂SO₄ + 2H₂O

From the balanced equation above,

Mole ratio of the acid, H₂SO₄ (nₐ) = 1

Mole ratio of the base, NaOH (n₆) = 2

Finally, we shall determine the molarity of the acid, H₂SO₄. This can be obtained as follow:

Volume of base, NaOH (V₆) = 38.70 cm³

Molarity of base, NaOH (M₆) = 1.90M

Volume of acid, H₂SO₄ (Vₐ) = 10.30 cm³

Molarity of acid, H₂SO₄ (Mₐ) =?

MₐVₐ / M₆V₆ = nₐ/n₆

Mₐ × 10.3 / 1.9 × 38.70 = 1/2

Mₐ × 10.3 / 73.53 = 1/2

Cross multiply

Mₐ × 10.3 × 2 = 73.53 × 1

Mₐ × 20.6 = 73.53

Divide both side by 20.6

Mₐ = 73.53 / 20.6

Mₐ = 3.57 M

Thus, the molarity of the acid, H₂SO₄ is 3.57 M

8 0
2 years ago
A mixture of He
aksik [14]

Answer : The partial pressure of nitrogen gas in the mixture is, 9.88 atm

Explanation :

According to the Dalton's Law, the total pressure of the gas is equal to the sum of the partial pressure of individual gases.

Formula used :

p_T=p_{He}+p_{Ar}+p_{N_2}

where,

p_T = total pressure of gas  = 13.6 atm

p_{He} = partial pressure of helium gas  = 1831 torr =  2.41 atm

p_{Ar} = partial pressure of argon gas  = 997 torr =  1.31 atm

Conversion used: (1 atm = 760 torr)

p_{N_2} = partial pressure of nitrogen gas  = ?

Now put all the given values in the above formula, we get:

13.6=2.41+1.31+p_{N_2}

p_{N_2}=9.88atm

Thus, the partial pressure of nitrogen gas in the mixture is, 9.88 atm

3 0
3 years ago
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