7 days ago

Al(s)+hcl(aq) → alcl3(aq)+h2(g). assume you have plenty of hcl and 6.0 mol of al. how many moles of h2 are formed?

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alisha [2963]

Answer:

180.56 kilojoules of heat energy is extracted when 1.00 kg of freon-11 evaporates.

Explanation:

The molar mass of freon-11 is 137.35 g/mol

The enthalpy of vaporization for freon-11 is 24.8 kJ/mol at its normal boiling point of 24°C. Given that, $\Delta H_{vap}=24.8 kJ/mol$

Mass of freon-11 evaporated = 1.00 kg = 1000 g

Moles of freon-11 evaporated can be calculated as

$\frac{1000 g}{137.35 g/mol}=7.2807 mol$

The energy removed in the form of heat when 1.00 kg of freon-11 vaporizes is:

$7.28067 mol\times \Delta H_{vap}=7.2807 mol\times 24.8 kJ/mol$

$=180.56 kJ$

0 0

2 months ago

Anarel [2989]

Answer:

The glycerol solution has a molality of 2.960×10^-2 mol/kg.

Explanation:

Calculating the moles of glycerol involves the formula: Moles = Molarity × Volume of solution = 2.950×10^-2 M × 1 L = 2.950×10^-2 moles.

To find the mass of water, use: Mass = Density × Volume = 0.9982 g/mL × 998.7 mL = 996.90 g, which converts to 0.9969 kg.

The formula for molality is: Molality = Moles of solute/Mass of solvent (in kg) = 2.950×10^-2/0.9969 = 2.960×10^-2 mol/kg.

7 0

3 months ago