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3 years ago

Aqueous solutions of Al(NO3)3 and KOH are mixed together. Identify the precipitate that will form.

1 answer:

8 0

The reaction between aluminium nitrate and potassium hydroxide will be given
by the equation;
Al(NO3)3 (aq) + KOH (aq) = KNO3 (aq) + Al(OH)3 (s)
Therefore, the precipitate resulting from the reaction is Aluminium hydroxide Al(OH)3.

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What is a metal and a non metal

Mrac [35]

Answer:

I assume you mean as in elements

A metal "A metal is a material that, when freshly prepared, polished, or fractured, shows a lustrous appearance, and conducts electricity and heat relatively well. Metals are typically malleable or ductile." (wiki)

a non-metal "In chemistry, a nonmetal is a chemical element that mostly lacks the characteristics of a metal. Physically, a nonmetal tends to have a relatively low melting point, boiling point, and density. A nonmetal is typically brittle when solid and usually has poor thermal conductivity and electrical conductivity." (wiki)

Explanation:

5 0

3 years ago

Read 2 more answers

When NH3(g) reacts with O2(g), the products of the combustion are NO(g) and H2O(g). What volume of O2(g) is required to react wi

arlik [135]

Answer: The volume of oxygen gas required is 3.75 mL

Explanation:

STP conditions:

1 mole of a gas occupies 22.4 L of volume.

We are given:

Volume of ammonia reacted = 3.00 mL = 0.003 L (Conversion factor: 1 L = 1000 mL)

The chemical equation for the reaction of ammonia with oxygen follows:

$4NH_3(g)+5O_2\rightarrow 4NO(g)+6H_2O(g)$

By Stoichiometry of the reaction:

(4 × 22.4) L of ammonia reacts with (5 × 22.4) L of oxygen gas

So, 0.003 L of ammonia will react with = $\frac{(5\times 22.4)}{(4\times 22.4)}\times 0.003=0.00375L=3.75mL$ of oxygen gas

Hence, the volume of oxygen gas required is 3.75 mL

4 0

3 years ago

consider the reaction between calcium oxide and carbon dioxide: cao ( s ) + co 2 ( g ) → caco 3 ( s ) a chemist allows 14.4 g of

MakcuM [25]

Answer:

CaO is the limiting reagent

Theoritical yield = 25.71 g

% Yield = 75.44%

Explanation:

1 mole = Molar mass of the substance

Molar Mass of CaO = 56 g/mol

Molar Mass of CaCO3 = 100 g/mol

Molar mass of CO2 = 44 g/mol

The balanced Equation is :

$CaO + CO_{2}\rightarrow CaCO_{3}$

1 mole of CaO reacts with = 1 mole of CO2

56 g of CaO reacts with = 44 g of CO2

1 g of CaO reacts with =

$\frac{44}{56}$

= 0.785 g of CO2

So,

14.4 g of CaO must react with = (14.4 x 0.785) g of CO2

= 11.31 g of CO2

Needed = 11.31 g

Available CO2 = 13.8 g (given)

So CO2 is in excess , hence CaO is the limiting reagent and product will produce from 14.4 g of CaO

$CaO + CO_{2}\rightarrow CaCO_{3}$

1 mole of CaO will produce 1 mole pf CaCO3

56 g of CaO produce = 100 g of CaCO3

1 g of CaO produce =

$\frac{100}{56}$

= 1.785 g of CaCO3

14.4 g of CaO will produce = (1.785 x 14.4) g of CaCO3

= 25.71 g of CaCO3

Theoritical Yield of CaCO3 = 25.71 g

Actual yield = 19.4 g

Percent Yield =

$\frac{Actual\ yield}{Theoritical\ yield}\times 100$

$\frac{19.4}{25.71}\times 100$

= 75.44 %

6 0

3 years ago

Can a compound have more than one carbon-carbon double bond in it?

kiruha [24]

Answer:

yes, a compound can have more than one carbon-carbon double bond

4 0

3 years ago

At catalyst is ______.

AlexFokin [52]

Heya!!!

Answer to your question:

A catalyst is ______
B. Not used up in a reaction.

Catalyst do not change the amount of reactants or products or itself get used but it just change the rate of reaction.

Hope it helps *_*

4 0

4 years ago