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pickupchik [31]
3 years ago
6

4.80 x 10^25 formula units pf calcium iodide (Cal2) will have what mass?

Chemistry
1 answer:
maw [93]3 years ago
7 0

Answer:

mass CaI2 = 23.424 Kg

Explanation:

From the periodic table we obtain for CaI2:

⇒ molecular mass CaI2: 40.078  + ((2)(126.90)) = 293.878 g/mol

∴ mol CaI2 = (4.80 E25 units )×(mol/6.022 E23 units) = 79.708  mol CaI2

⇒ mass CaI2 = (79.708 mol CaI2)×(293.878 g/mol) = 23424.43 g

⇒ mass CaI2 = 23.424 Kg

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Explanation:

2. 2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O

First, we need to find the number of moles of CO_2 at 300K and 1.5 atm using the ideal gas law:

n= \dfrac{PV}{RT}= \dfrac{(1.5\:\text {atm})(33\:L)}{(0.082\:\text{L-atm/mol-K})(300K)}

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2.0\:\text{mol}\:CO_2 \times \left(\dfrac{2\:\text{mol}\:C_2H_6}{4\:\text{mol}\:CO_2}\right)

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Finally, convert this amount to grams using its molar mass:

1.0\:\text {mol}\:C_2H_6 \times \left(\dfrac{30.07\:\text g\:C_2H_6}{1\:\text{mol}\:C_2H_6} \right)

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3. 3Zn + 2H_3PO_4 \rightarrow 3H_2 + Zn_3(PO_4)_2

Convert 75 g Zn into moles:

75\:\text g\:Zn \times \left(\dfrac{65.38\:\text g\:Zn}{1\:\text{mol}\:Zn}\right)=1.1\:\text{mol}\:Zn

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1.1\:\text{mol}\:Zn \times \left(\dfrac{3\:\text{mol}\:H_2}{3\:\text{mol}\:Zn}\right)=1.1\:\text{mol}\:H_2

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V= \dfrac{nRT}{P}= \dfrac{(1.1\:\text{mol}\:H_2)(0.082\:\text{L-atm/mol-K})(296K)}{4\:\text{atm}}

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In a unimolecular reaction with twice as much starting material as product at equilibrium, what is the value of Keq? Is ΔG o pos
lubasha [3.4K]

Answer : The value of K_{eq} is, 0.5 and \Delta G= positive.

Explanation :

The unimolecular reaction is:

A\rightarrow B

In unimolecular reaction, the starting material is 2 times to the product.

A=2B      .........(1)

As we know that:

K_{eq}=\frac{B}{A}     ...........(2)

Now substitute equation 1 in 2, we get:

K_{eq}=\frac{\frac{A}{2}}{A}

K_{eq}=0.5

Now we have to calculate the value of \Delta G^o at 298 K.

\Delta G^o=-RT\ln K_{eq}

where,

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

R = gas constant = 8.314 J/mol.K

T = temperature = 298 K

K_{eq} = equilibrium constant = 0.5

Now put all the given values on the above formula, we get:

\Delta G^o=-(8.314J/mol.K)\times (298K)\ln (0.5)

\Delta G^o=1717.32J/mol

Thus, the value of \Delta G^o at 298 K is, 1717.32 J/mol

As we know that:

\Delta G= +ve, reaction is non spontaneous

\Delta G= -ve, reaction is spontaneous

\Delta G= 0, reaction is in equilibrium

Thus, the \Delta G= +ve. So, the reaction is non spontaneous.

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