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2 years ago

Calculate the volume of "dry" hydrogen that would be produced by one mole of magnesium at

Chemistry

1 answer:

kakasveta [241]2 years ago

5 0

Answer:The volume of H2 = 243mL = 0.243 L

Pressure of H2 gas collected = 745 mm

Pressure of H2 dry gas = P of H2 collected - vapor pressure of water = 745- 23.78 = 721.22 mm

= 721.22mm /760mm/atm

Temperature = 25C = 25+273= 298 K

Using the ideal gas equation

PV = nRT

or PV = (mass/molar mass) RT

(721.22/760)atm x 0.243L = (mass/ 2g/mol) x 0.0821L.atm/mol.K x 298K

Thus mass of H2 formed = 0.0188 g

Explanation:

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What is the molality of a solution that is obtained by dissolving 2.922 g of NaCl into 1000.0 g of water if the molar mass of Na

never [62]

In order to find molarity, you must first find the number of moles that was dissolved.

Now, Moles = Mass ÷ Molar Mass

⇒ Moles of NaCl = 2.922 g ÷ 58.44 g/mol

= 0.05 moles

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4 0

3 years ago

Answer question 13. What is the mechanical advantage of a lever that can lift a 100 N load with a input force of 20 N

vazorg [7]

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3 years ago

In an equimolar mixture of o2 and n2, are the mass fractions equal?

nika2105 [10]

Answer:

Explanation:

The mass fraction is defined as:

$w_{i}=\frac{m_{i} }{m_{t} }$

where:

wi: mass fraction of the substance i
mi: mass of the substance i
mt: total mass of the system

The mass fraction of two substances (A and B), will be the same, ONLY if the mass of the substance A (mA) is the same as the mass of the substance B (mB).

An equimolar mixutre of O2 and N2 has the same amount of moles of oxygen and nitrogen, just to give an example let's say that the system has 1 mole of O2 and 1 mole of N2. Then using the molecuar weigth of each of them we can calculate the mass:

mA= 1 mole of O2 * 16 g/1mol = 16 g

mB=1 mole of N2 *28 g/1mol=28 g

As mA≠mB then the mass fractions are not equal, so the answear is NO.

4 0

3 years ago

??????????????? why ????????????????

stealth61 [152]

Answer:

because

Explanation:

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3 years ago

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3 years ago