Answer : The pressure in torr and in atmospheres are, 745 torr and 0.980 atm respectively.
Explanation :
As we are given that the atmospheric pressure is, 745 mmHg.
Now we have to determine the pressure in torr and atm.
Conversions used:
1 atm = 760 mmHg
1 atm = 760 torr
1 mmHg = 1 torr
As, 760 mmHg = 1 atm
So, 745 mmHg = ![\frac{745mmHg}{760mmHg}\times 1atm=0.980atm](https://tex.z-dn.net/?f=%5Cfrac%7B745mmHg%7D%7B760mmHg%7D%5Ctimes%201atm%3D0.980atm)
and,
As, 1 mmHg = 1 torr
So, 745 mmHg = 745 torr
Therefore, the pressure in torr and in atmospheres are, 745 torr and 0.980 atm respectively.
Answer:
- 13,150.6kJ
Explanation:
CH4 + 2 O2 ------> CO2 + 2 H2O ΔH= – 890 kJ
The ΔH is enthalpy change of combustion , which is the heat is either absorbed or released by the combustion of one mole of a substance.
ΔH=−890 kJ/mol (released in the combustion of one mole of methane)
using the molar mass (in grams )of methane to get moles of sample
(237g × 1 mole of CH4)/16.04g=14.776 moles of CH4
Since 1 mole produces 890 kJ of heat upon combustion, then 14.776 moles will produce
ΔH = 14.776moles of CH4 × 890kJ/1mole of CH4
=13,150.6kJ
Therefore ΔH = - 13,150.6kJ
Answer: Balance (B.)
Explanation:
Balances are used to measure mass.
Beakers and graduated cylinders measure volume. Stopwatches measure time. Meter sticks measure length. Thermometers measure temperature.
Answer:
Covalent
Explanation:
Covalent is the sharing of electrons and Ionic is transferring of electrons.
133.0873 g/mol
(NH4)3PO3 - molar mass