Answer:
the rate of heat required is 38185,056 J/h
Explanation:
for gases, heat is given for the expresion:
∴ T1 = 43°C + 273 = 316 K
∴ T2 = 225°C + 273 = 498 K
⇒ ΔT = T2 - T1 = 498 - 316 = 182 K
∴ Cp HBr (298 K) = 29.14 J / mol * K.......specific heat tables
⇒ Q = (7.2 mol/h ) * (29.14 J/mol K) * ( 182 K )
⇒ Q = 38185.056 J/h
Answer:
24dm³
Explanation:
Given parameters:
Mass of CO = 30g
Unknown:
Volume of CO at STP = ?
Solution:
To solve this problem, we need to find the number of moles of CO in the given mass.
Number of moles of CO =
Molar mass of CO = 12 + 16 = 28g/mol
Number of moles = = 1.07moles
Now;
1 mole of a gas occupies 22.4dm³ volume at STP
1.07moles will occupy 1.07 x 22.4 = 24dm³
The molarity of a solution equals to the mole number of the solute/the volume of the solution. For NH4Br, we know that the mole mass is 98. So the molarity is (14/98) mol /0.15 L=0.95 mol/L.
Missing question: <span> The vapor pressure of water at 26.4 °C is 25.81 mm Hg.
p(total) = p(H</span>₂O) + p(O₂).
p(total) = 817 torr; <span> total pressure of the mixture.
</span>p(H₂O) = 25.81 torr, <span>partial pressure of water.
</span>p(O₂) = 817 torr - 25.81.
p(O₂) = 791.19 torr; partial pressure of oxygen.