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2 years ago

A solution with a pH = 13 has approximately how many moles of OH– ions per liter?

Chemistry

1 answer:

FrozenT [24]2 years ago

3 0

Answer:

1 × 10-¹ moldm-³

Explanation:

Pkw = PH + POH

14 = 13 + POH

POH = 1

so , [OH-] = 1 × 10-¹ moldm-³

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B) Methanoic Acid

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Which group on the periodic table already stable?

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The noble gases AKA the column with full outermost valence shells. (Group 18)

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3 years ago

Balance the following reaction in KOH (under basic conditions). What are the coefficients in for C3H8O2 and KMnO4 in the balance

GrogVix [38]

Answer:

Coefficient of $C_3H_8O_2=3$

Coefficient of $KMnO_4$ =8

Explanation:

We are given that a reaction in which $C_3H_8O_2$ reacts with $KMnO_4$

We have to find the coefficient of each reactants in balanced reaction

$3C_3H_8O_2(aq)+8KMnO_4(aq)\rightarrow 3C_3H_2O_4K_2(aq)+8MnO_2(aq)+2KOH+8H_2O$

Coefficient is defined the constant value multiplied with a reactant in a reaction.

Coefficient of $C_3H_8O_2$ =3

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Coefficient of $MnO_2=8$

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Hence, Coefficient of $C_3H_8O_2=3$ and coefficient of $KMnO_4=8$

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3 years ago

For the following reaction, 5.04 grams of nitrogen gas are allowed to react with 8.98 grams of oxygen gas: nitrogen(g) + oxygen(

OLga [1]

Answer:

1. 10.8 g of NO

2. N₂ is the limting reagent

3. 3.2 g of O₂ does not react

Explanation:

We determine the reaction: N₂(g) + O₂(g) → 2NO(g)

We need to determine the limiting reactant, but first we need the moles of each:

5.04 g / 29 g/mol = 0.180 moles N₂

8.98 g / 32 g/mol = 0.280 moles O₂

Ratio is 1:1, so the limiting reactant is the N₂. For 0.280 moles of O₂ I need the same amount, but I only have 0.180 moles of N₂

Ratio is 1:2. 1 mol of N₂ can produce 2 moles of NO

Then, 0.180 moles of N₂ may produce (0.180 .2) / 1 = 0.360 moles NO

If we convert them to mass → 0.360 mol . 30 g/1 mol = 10.8 g

As ratio is 1:1, for 0.180 moles of N₂, I need 0.180 moles of O₂.

As I have 0.280 moles of O₂, (0.280 - 0.180 ) = 0.100 moles does not react.

0.1 moles . 32 g/mol = 3.2 g of O₂ remains after the reaction is complete.

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3 years ago

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