The answer for the following question is answered below.
- <em><u>Therefore the new pressure of the gas is 1.76 atm.</u></em>
Explanation:
Given:
Initial pressure of the gas = 1.34 atm
Initial temperature of the gas = 273 K
final temperature of the gas = 312 K
To solve:
Final temperature of the gas
We know;
From the ideal gas equation
P × V = n × R × T
So;
from the above equation we can say that
<em>P ∝ T</em>
= constant
=
Where;
= initial pressure of a gas
= final pressure of a gas
= initial temperature of a gas
= final temperature of a gas
=
= 1.76 atm
<em><u>Therefore the new pressure of the gas is 1.76 atm.</u></em>
Answer:
5 L.
Explanation:
From the question given above, the following data were obtained:
Initial volume (V1) = 10 L
Initial pressure (P1) = 2.5 atm
Final pressure (P2) = 5 atm
Final volume (V2) =.?
Since the temperature is constant, we shall apply the Boyle's law equation to determine the new volume of the gas. This can be obtained as follow:
P1V1 = P2V2
2.5 × 10 = 5 × V2
25 = 5 × V2
Divide both side by 5
V2 =25/5
V2 = 5 L
Thus, the new volume of the gas is 5 L
Answer:
see explanation
Explanation:
a. Molar Mass = ∑Atomic Masses = 12C + 22H + 11O = 12(12) + 22(1) + 11(16) = 144 + 22 + 176 = 342 g/mole
b. For 100ml of 0.10M solution => Molarity x Volume (liters) = moles needed x mole weight = grams solute needed for 100ml solution. This can be given by the expression ...
mass solute needed (g) = Molarity needed x Volume needed in liters x mole wt of solute = (0.10M)(0.100L)(342g/mole) = 3.42 grams solute.
mixing => Transfer 3.42 grams of solute (C₁₂H₂₂O₁₁) into mixing container and add solvent (water) up to but not to exceed 100 ml total volume.
c. mass needed for 100ml of 0.50M solution = M·V·f.wt. = (0.50M)(0.100L)(342g/mole) = 1.71 grams solute. => mix as in 'b'.