Answer:
T2 = 260 K
Explanation:
<em>Given data:</em>
P1 = 150.0 k Pa
T1 = (-23+ 273.15) K = 250.15 K
V1 = 1.75 L
P2 = 210.0 kPa
V2 = 1.30 L
<em>To find:</em>
T2 = ?
<em>Formula:</em>
<em>Calculation:</em>
T2 = (210.0 kPa) x (1.30 L) x (250.15 K) / (150.0 kPa) x (1.75 L)
T2 = 260 K
We have to know the number of molecules present in 500 g of water.
The answer is: zero molecules present in 500g of water.
Water molecule is H₂O. In water molecule, nitrogen molecule can not be present. Molecular mass of water is 18 g. MOlecular mass of nitrogen molecule is 28 g.
500 g water contains 500/18 number of moles= 27.77 moles of water molecules which contains 27.77 X 6.023 X 10²³ number of water molecules.
There is no existence of N₂ molecule.
Answer: D. The number of molecules having Er or greater doubles.
Explanation: As the temperature increases from 20°C to 30°C, the number of molecules with maximum energy decreases, but the number of effective collisions which result into the formation of product doubles.
This is due to doubling of molecules which possess energy equal to or greater than 
which means now double number of molecules will be able to cross the energy barrier and hence the formation of product increases and hence the rate increases to double.
Because of the motion, the faster the particles move , the higher temperature goes
Answer:
1.38 mol.
Explanation:
- It is known that every 1.0 mole of a molecule contains Avogadro's number of molecules (NA = 6.022 x 10²³).
<em><u>Using cross multiplication:</u></em>
1.0 mole of H₂SO₄ contains → 6.022 x 10²³ molecules.
??? moles of H₂SO₄ contains → 8.31 x 10²³ molecules.
<em>∴ The no. of moles in (8.31 x 10²³ molecules) of H₂SO₄ </em>= (1.0 mol)(8.31 x 10²³) / (6.022 x 10²³ molecules) = <em>1.38 mol.</em>
