Answer:
3.59 moles
Explanation:
Hopefully this helps! :)
Mark as brainliest if right!
Answer:
The volume is 1.2L
Explanation:
Initial volume (V1) = 700mL = 0.7L
Initial temperature (T1) = 7°C = (7 + 273.15)K = 280.15K
Initial pressure = 106.6kPa = 106600Pa
Final temperature (T2) = 27°C = (27 + 273.15)K = 300.15K
Final pressure (P2) = 66.6kPa = 66600Pa
Final volume (V2) = ?
To solve this question, we need to use combined gas equation which is a combination of Boyle's law, Charles Law and pressure law.
(P1 × V1) / T1 = (P2 × V2) / T2
solve for V2 by making it the subject of formula,
P1 × V1 × T2 = P2 × V2 × T1
V2 = (P1 × V1 × T2) / (P2 × T1)
V2 = (106600 × 0.7 × 300.15) / (66600 × 280.15)
V2 = 22397193 / 18657990
V2 = 1.2L
The final volume of the gas is 1.2L
Answer:
Ca(NO3)2 has the highest boiling point ( option A)
Explanation:
Step 1: Data given
A. 1.25 M Ca(NO3)2
B. 1.25 M KNO3
C. 1.25 M CH3OH
D. 2.50 M C6H12O6
Step 2: Calculate highest boiling point
The boiling point depends on the van't Hoff factor
This shows the particles produced when the substance is dissolved. For non-electrolytes dissolved in water, the van' t Hoff factor is 1.
Ca(NO3)2 → Ca^2+ + 2NO3- → Van't Hoff factor = 3
KNO3 → K+ + NO3- → Van't Hoff factor = 2
CH3OH is a non-elektrolyte → Van't Hoff factor = 1
C6H12O6 is a non-elektrolyte → Van't Hoff factor = 1
Ca(NO3)2 has the highest boiling point
<h3>
Answer:</h3>
1.25 moles (R.T.P.) or 1.34 moles (S.T.P.)
<h3>
Explanation:</h3>
- 1 mole of a gas occupies a volume of 24 liters at room temperature and pressure (R.T.P.)
- On the other hand, 1 mole of a gas will occupy 22.4 Liters at standard temperature and pressure (S.T.P.)
Therefore, at R.T.P.
30.0 Liters will be equivalent to;
= 30.0 L ÷ 24 L
= 1.25 moles
At S.T.P
30.0 Liters will be equivalent to;
= 30.0 L ÷ 22.4 L
= 1.34 moles
Thus, 30.0 L of helium gas are equivalent to 1.25 moles of He at R.T.P. and 1.34 moles at S.T.P.
