1.0 mg/mL
a) Convert <em>grams to milligrams
</em>
Mass = 1.0 g × (1000 mg/1 g) = 1000 mg
b) Convert <em>litres to millilitres
</em>
Volume = 1 L × (1000 mL/1 L) = 1000 mL
c) Calculate the <em>density
</em>
ρ = mass/volume = 1000 mg/1000 mL = 1.0 g/mL
Answer: 3 moles solute x 1 dm^3/0.60 moles solute = 5 dm^3
Explanation:
The ideal gas model assumes that gas particles experience no intermolecular attractions.
At low temperature, gas particles move slowly.
At high pressures, gas particles are very close together.
The closeness of the gas particles and their low speed allow intermolecular forces to become important at high pressure and low temperature.
The intermolecular forces cause the gas to deviate from ideal behavior.
Here we have to get the amount of heat will generate by 510.0 kg of sodium sulfate decahydrate at night assuming complete reaction and 100% efficiency of heat transfer.
510.0 kg of sodium sulfate decahydrate will produce 5.603 × 10⁵ kJ of heat energy.
The molecular weight of sodium sulfate decahydrate (H₂₀Na₂O₁₄S) 322.186 g/mol.
Thus 510.0 kg of H₂₀Na₂O₁₄S is equivalent to = 1582.936 mol of H₂₀Na₂O₁₄S.
Now per mole of H₂₀Na₂O₁₄S will transfer 354 kJ heat.
Thus 1582.936 mol will transfer 1582.936 × 354 kJ = 5.603×10⁵ kJ of heat.
Henceforth, 510.0 kg of sodium sulfate decahydrate will produce 5.603 × 10⁵ kJ of heat energy.
Answer: B. HCl(g)+H2O(I)—>H3O+(aq)+Cl-(aq)
D. CO2(g)+2H2O(I)—>HCO3-(aq)+H3O+(aq)
Explanation: on edge