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2 years ago

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A chemist determines by measurements that moles of nitrogen gas participate in a chemical reaction. Calculate the mass of nitrog

en gas that participates.

1 answer:

Likurg_2 [28]2 years ago

4 0

Answer:

0.56 g

Explanation:

<em>A chemist determines by measurements that 0.020 moles of nitrogen gas participate in a chemical reaction. Calculate the mass of nitrogen gas that participates.</em>

Step 1: Given data

Moles of nitrogen gas (n): 0.020 mol

Step 2: Calculate the molar mass (M) of nitrogen gas

Molecular nitrogen is a gas formed by diatomic molecules, whose chemical formula is N₂. Its molar mass is:

M(N₂) = 2 × M(N) = 2 × 14.01 g/mol = 28.02 g/mol

Step 3: Calculate the mass (m) corresponding to 0 0.020 moles of nitrogen gas

We will use the following expression.

m = n × M

m = 0.020 mol × 28.02 g/mol

m = 0.56 g

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Use the provided reduction potentials to calculate ArGº for the following balanced redox reaction: Pb2+(aq) + Cu(s) → Pb(s) + Cu

nydimaria [60]

Answer : The correct option is, +91 kJ/mole

Solution :

The balanced cell reaction will be,

$Cu(s)+Pb^{2+}(aq)\rightarrow Cu^{2+}(aq)+Pb(s)$

Here copper (Cu) undergoes oxidation by loss of electrons, thus act as anode. Lead (Pb) undergoes reduction by gain of electrons and thus act as cathode.

First we have to calculate the standard electrode potential of the cell.

$E^0_{[Pb^{2+}/Pb]}=-0.13V$

$E^0_{[Cu^{2+}/Cu]}=+0.34V$

$E^0_{cell}=E^0_{cathode}-E^0_{anode}$

$E^0_{cell}=E^0_{[Pb^{2+}/Pb]}-E^0_{[Cu^{2+}/Cu]}$

$E^0_{cell}=-0.13V-(0.34V)=-0.47V$

Now we have to calculate the standard Gibbs free energy.

Formula used :

$\Delta G^o=-nFE^o_{cell}$

where,

$\Delta G^o$ = standard Gibbs free energy = ?

n = number of electrons = 2

F = Faraday constant = 96500 C/mole

$E^o$ = standard e.m.f of cell = -0.47 V

Now put all the given values in this formula, we get the Gibbs free energy.

$\Delta G^o=-(2\times 96500\times (-0.47))=+90710J/mole=+90.71kJ/mole\approx +91kJ/mole$

Therefore, the standard Gibbs free energy is +91 kJ/mole

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2 years ago

How many moles of magnesium, Mg, are there in 4.75 grams of magnesium?

Nina [5.8K]

Molar mass Mg = 24.3 g/mol

1 mole mg ------------ 24.3 g
?? moles mg --------- 4.75 g

4.75 x 1 / 24.3 => 0.195 moles of Mg

hope this helps!

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2 years ago

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azamat

Answer:

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Explanation:

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2 years ago

Read 2 more answers

Two systems with heat capacities 19.9 J mol-1 K-1 and 28.2 ] mol 1 K-1 respectively interact thermally and come to an equilibriu

MAVERICK [17]

Answer : The initial temperature of system 2 is, $19.415^oC$

Explanation :

In this problem we assumed that the total energy of the combined systems remains constant.

$-q_1=q_2$

$m\times c_1\times (T_f-T_1)=-m\times c_2\times (T_f-T_2)$

The mass remains same.

where,

$C_1$ = heat capacity of system 1 = 19.9 J/mole.K

$C_2$ = heat capacity of system 2 = 28.2 J/mole.K

$T_f$ = final temperature of system = $30^oC=273+30=303K$

$T_1$ = initial temperature of system 1 = $45^oC=273+45=318K$

$T_2$ = initial temperature of system 2 = ?

Now put all the given values in the above formula, we get

$-19.9J/mole.K\times (303-318)K=28.2J/mole.K\times (303-T_2)K$

$T_2=292.415K$

$T_2=292.415-273=19.415^oC$

Therefore, the initial temperature of system 2 is, $19.415^oC$

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3 years ago

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larisa86 [58]

Answer:

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Explanation:

Im not 100% sure if this is correct!

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2 years ago