Following are the Balanced Reactions,
Reaction 1:
(NH₄)₂CO₃ → <u>2</u> NH₄⁺ + CO3⁻²
Reaction 2:
PbI₂ → Pb⁺²<span> + <u>2</u> I</span>⁻¹
Reaction 3:
<span>(NH</span>₂<span>)</span>₃<span>PO</span>₄ → <span><u>3</u> NH</span>₄⁺ <span>+ PO</span>₄⁻³
The answer to your question would be _B High Temp
Answer:
Solution of isopropanol is 10.25 molal
Explanation:
615 g of isopropanol (C3H7OH) per liter
We gave the information that 615 g of solute (isopropanol) are contained in 1L of water. We need to find out the mass of solvent, so we use density.
Density of water 1g/mL → Density = Mass of water / 1000 mL of water
Notice we converted the L to mL
Mass of water = 1000 g (which is the same to say 1kg)
Molality are the moles of solute in 1kg of solvent, so let's convert the moles of isopropanol → 615 g . 1mol / 60g = 10.25 moles
Molality (mol/kg) = 10.25 moles / 1kg = 10.25 m
