Explanation:
Step 1:
Data obtained from the question. This include the following:
Initial pressure (P1) = 1atm
Initial temperature (T1) = 0°C = 0°C + 273 = 273K
Final temperature (T2) = 280°C = 280°C + 273 = 553K
Final pressure (P2) =...?
Step 2:
Determination of the new pressure of the gas.
Since the volume of the gas is constant, the following equation:
P1/T1 = P2/T2
will be used to obtain the pressure. This is illustrated below:
P1/T1 = P2/T2
1/273 = P2 / 553
Cross multiply
273x P2 = 553
Divide both side by 273
P2 = 553/273
P2 = 2.03atm
Therefore, the new pressure of the gas will be 2.03atm
Answer:
612 K
Explanation:
From the question given above, the following data were obtained:
Initial temperature (T₁) = 306 K
Initial pressure (P₁) = 150 kPa
Final pressure (P₂) = 300 kPa
Volume = 4 L = constant
Final temperature (T₂) =?
Since the volume is constant, the final (i.e the new) temperature of the gas can be obtained as follow:
P₁ / T₁ = P₂ / T₂
150 / 306 = 300 / T₂
Cross multiply
150 × T₂ = 306 × 300
150 × T₂ = 91800
Divide both side by 150
T₂ = 91800 / 150
T₂ = 612 K
Thus, the new temperature of the gas is 612 K
1) moles = mass/mR
CaCO3 Mr = 40 + 12 + (16×3)
= 52 + 48
= 100
mass = 15
so the moles would be 15 ÷ 100
which is 0.15 moles of CaCO3
2) moles = mass ÷ Mr
Mr of Al2O3 = 27 + (16×3)
= 27 + 48
= 75
mass = 204
so the moles would be 204/75 which is 2.72 moles of Al2O3
Answer:
308,4796 g.
Explanation:
1 mol equals to 107,86 g, now times 2,86 mol, 308,4796 g.
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