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2 years ago

Write a balanced chemical equation showing how each metal oxide reacts with HCl.

Chemistry

1 answer:

larisa86 [58]2 years ago

3 0

Answer:

ZnO(s) + 2HCl(aq) ------> ZnCl2(aq) + H2O(l)

Na2O(s) + 2HCl(aq) -----> 2NaCl(aq) + H2O(l)

Rb2O(s) + 2HCl(aq) -----> 2RbCl(aq) + H2O(l)

NiO(s) + 2HCl(aq) --------> NiCl2(aq) + H2O(l)

MgO(s) + 2HI(aq) -----> MgI2(aq) + H2O(l)

Na2O(s) + 2HI(aq) -----> 2NaI(aq) + H2O(l)

CaO(s) + 2HI(aq) ----> CaI2(aq) + H2O(l)

Explanation:

Let us recall that the oxides of metals are basic in nature. These basic metal oxides can react with acids to form salt and water only.

In the reactions above, HCl and HI were reacted with different metal oxides and the corresponding salts of each metal and water was formed as shown.

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Giving out 15 free pts bc im in a good mood :)

Artemon [7]

Answer:

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2 years ago

PLEASE HELP IM SO CONFUSED How does potassium need to be modified either on site or in a factory to make it useful. This should

3241004551 [841]

Potassium is not found free in nature but is found in the form of potash. Potash is the ore of potassium and this ore is mined from deep down the earth or can sometimes be found on the surface. Potash was mostly formed as sea water receded and left deposits.

Potash is usually in the form of potassium salts such potassium chloride and potassium sulphate. The potash is mined then taken to the factory where it is crushed and purified by removing such impurities as clay.

The now purified potassium salts are subjected to a process called electrolysis where potassium metal is obtained from its salt.

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3 years ago

5.1169 mol of Ne is held at 0.9148 atm and 911 K. What is the volume of its container in liters?

sveticcg [70]

By applying the Boyle's equation and substituting our given data the volume of the container was found to be 418.14 Litres

<h3>Boyle's Law</h3>

Given Data

number of moles of Ne = 5.1169 mol

Pressure = 0.9148 atm

Temperature = 911 K

We know that the relationship between pressure and temperature is given as

PV = nRT

R = 0.08206

Making the volume subject of formula we have

V= nRT/P

Substituting our given data to find the volume we have

V = 5.1169*0.08206*911/0.9148

V = 382.522353554/0.9148

V = 418.14 L

Learn more about Boyle's law here:

brainly.com/question/469270

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1 year ago

PLS HURYYY ILL GIVE BRAINLIEST

ad-work [718]

The volume increases when the balloon temperature increases.

<u>Explanation:</u>

-10 F is converted into Kelvin as 249 K.

0°C is nothing but 0+ 273 = 273 K

And the room temperature is 25°C which is converted into Kelvin as 273 + 25 = 298 K.

249 K is below room temperature.

As per the Charles' law volume and temperature are directly proportional to each other, when the pressure of the gas remains constant.

V ∝ T

As the balloon temperature increases, the volume also increases.

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3 years ago

At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L . What volume wo

Nostrana [21]

Taking into account the Charles's law, the same amount of gas at the same pressure and 65 ∘C would occupy a volume of 27.73 L.

<h3>Charles's Law</h3>

Charles's Law consists of the relationship that exists between the volume and the temperature of a certain quantity of ideal gas, at a constant pressure.

Volume is directly proportional to the temperature of the gas: if the temperature increases, the volume of the gas increases, while if the temperature of the gas decreases, the volume decreases.

Mathematically, Charles's law is a law that says that the quotient that exists between the volume and the temperature will always have the same value:

V÷ T= k

Considering an initial state 1 and a final state 2, it is satisfied:

V1÷ T1= V2÷ T2

<h3>Volume at 65°C</h3>

In this case, you know:

V1= 22.4 L
T1= 0 C= 273 K
V2= ?
T2= 65 C= 338 K

Replacing in Charles's law:

22.4 L÷ 273 K= V2÷ 338 K

Solving:

(22.4 L÷ 273 K) ×338 K= V2

Finally, the same amount of gas at the same pressure and 65 ∘C would occupy a volume of 27.73 L.

Learn more about Charles's law:

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#SPJ1

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1 year ago