Answer:
When 0.250 moles of a gas is placed in a container at 25 °C, it exerts a pressure of 700 mm Hg.
Explanation:
Answer:
18.06 g of ammonia
Explanation:
This is the reaction:
NH₃ + CH₃OH → CH₃NH₂ + H₂O
Ratio is 1:1
1 mol of ammonia reacts with 1 mol of methanol.
Let's convert the mass of methanol to moles.
34 g . 1 mol / 32 g = 1.06 moles
We need 1.06 moles of NH₃ whichs is the same to say:
1.06 moles. 17 g / 1 mol = 18.06 g of NH₃
H- is the one without electron
Answer:
The temperature of the methanol will increase more rapidly.
Explanation:
The premise of your question is incorrect. Methanol has an OH group, so there ARE hydrogen bonds among methanol molecules.
However, the specific heat capacity of methanol is 2.53 J°C⁻¹g⁻¹, while that of water is 4.18 J°C⁻¹g⁻¹.
Thus, it takes 65 % more heat energy to raise the temperature of a given mass of water by 1 °C than it does to raise the temperature of an equal mass of methanol by the same amount.
The two samples are receiving heat energy at the same rate, so the methanol will heat up faster than the water.