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Gwar [14]
3 years ago
6

Write a balanced molecular equation for hydrochloride acid solution combined with a potassium hydroxide solution, an acid base r

eaction occurs
Chemistry
1 answer:
qaws [65]3 years ago
7 0

Answer:

HCl (aq) + KOH (aq) --------> KCl (aq) + H2O (l)   [balanced molecular equation]

Explanation:

Balanced molecular equation has all the components of reaction written as "molecules" thus the name molecular (the other equations break appropriate components into ions, those are total ionic or net ionic equation)

We know hydrochloride acid solution is written as HCl (aq) and potassium hydroxide solution is written as KOH (aq). We know from our knowledge that when acids react with bases they make salt and water, so now we react!

HCl (aq) + KOH (aq) --------> KCl (aq) + H2O (l)   [balanced molecular equation]

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4 years ago
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Dwayne filled a small balloon with air at 298.5 K. He put the balloon into a bucket of water, and the water level in the bucket
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Answer : The volume of the balloon will be, 0.494 liters

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Charles' Law : It is defined as the volume of the gas is directly proportional to the temperature of the gas at constant pressure and number of moles.

V\propto T

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\frac{V_1}{T_1}=\frac{V_2}{T_2}

where,

V_1 = initial volume of gas = ?

V_2 = final volume of gas = 0.54 L

T_1 = initial temperature of gas = 273.15 K

T_2 = final temperature of gas = 298.5 K

Now put all the given values in the above equation, we get the initial volume of balloon.

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HELPPP!!! What is the volume of a 1.31 moles sample of gas if the pressure is 904 mmHg and the temperature is 37. degrees Celsiu
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Answer:

27.99 dm³

Explanation:

Applying

PV = nRT................ Equation 1

Where P = Pressure, V = Volume, n = number of mole, R = molar gas constant, T = Temperature.

From the question, we were aksed to find V.

Therefore we make V the subject of the equation

V = nRT/P................ Equation 2

Given: n = 1.31 moles, T = 37°C = 310K, P = 904 mmHg = (904×0.001316) = 1.1897 atm

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Substitute these values into equation 2

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