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MrMuchimi
3 years ago
12

How many moles of chlorine (Cl) atoms are in a sample of 1.72 × 1022 atoms? 0.0286 mol Cl 35.0 mol Cl 1.03 × 1023 mol Cl 1.04 ×

1046 mol Cl
Chemistry
1 answer:
kogti [31]3 years ago
6 0

Given information : Sample of 1.72\times 10^{22} atoms

We need to find the moles of Chlorine in the given sample.

We can say that we need to find moles from the given atoms.

Relation between mole and atom is given by : 1 mole = 6.022\times 10^{23} atoms

Where 6.022\times 10^{23} is Avogadro number.

1.72\times 10^{22} atoms\times \frac{1 mole}{6.022\times 10^{23} atoms}

1.72\times 10^{22}\times \frac{1 mole}{6.022\times 10^{23}}

On solving the above equation , atoms(unit) gets cancelled out and we get 0.0286 mol.

In the given sample the moles of Chlorine (Cl) is 0.0286 mol , so option A is correct.

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Nimfa-mama [501]

Answer: 4.18925 kJ heat is needed to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -50°C.

Explanation:

Temperature of Solid C_2H_5OH=-135^oC=138 K(0^oC=273K)

Melting temperature of Solid C_2H_5OH=114^oC=159 K

Temperature of liquid C_2H_5OH=-50^oC=223K

Specific heats of solid  ethanol = 0.97 J/gK

Specific heats of liquid ethanol = 2.3 J/gK

Heat required to melt the the 25 g solid C_2H_5OH at 159 K

\Delta T_1 = 159 K - 138 K = 21 K

Q_1=mc\Delta T= 25\times 0.97J/gK\times 21 K=509.25 J

Heat required to melt and raise the temperature of C_2H_5OH upto 223 K

\Delta T_2 = 223 K - 159 K  = 64 K

Q_2=mc\Delta T= 25\times 2.3J/gK\times 64 K=3680 J

Total heat to convert solid ethanol to liquid ethanol at given temperature :

Q_1+Q_2=509.25 J+3680 J=4189.25 J=4.18925 kJ (1kJ=1000J)

Hence, 4.18925 kJ of heat will be required to convert 25.0 g of solid ethanol at -135 °C to liquid ethanol at -50°C.

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This question is incomplete without the table

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The missing table is attached to this answer.

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The charge of an electron was first determined by R. Milikan using the oil-drop experiment

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The charge of a neutron was first determined by (or credited to) James Chadwick.

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The mass of an electron was first measured by J. J. Thomson.

The mass of a proton was first measured by (or credited to) Ernest Rutherford.

The mass of a neutron was first measured by James Chadwick.

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