Answer:
1.78 atm
Explanation:
From the question given above, the following data were obtained:
Mass of Cl = 355 g
Molecular weight of Cl = 70.9 g/mol
Volume (V) = 70.0 L
Temperature (T) = 30 °C
Pressure (P) =?
Next, we shall determine the number of mole in 355 g of chlorine (Cl). This can be obtained as follow:
Mass of Cl = 355 g
Molecular weight of Cl = 70.9 g/mol
Mole of Cl =.?
Mole = mass /molecular weight
Mole of Cl = 355 /70.9
Mole of Cl = 5 moles
Next, we shall convert 30 °C to Kelvin temperature. This can be obtained as follow:
T(K) = T(°C) + 273
Temperature (T) = 30 °C
Temperature (T) = 30 °C + 273 = 303 K
Finally, we shall determine the pressure of the gas as illustrated below:
Volume (V) = 70.0 L
Number of mole (n) = 5 moles
Temperature (T) = 303 K
Gas constant (R) = 0.0821 atm.L/Kmol
Pressure (P) =?
PV = nRT
P × 70 = 5 × 0.0821 × 303
P × 70 = 124.3815
Divide both side by 70
P = 124.3815 / 70
P = 1.78 atm
Therefore, the pressure of the gas is 1.78 atm
The chemical formula of chromium (II) nitrate is as shown below.
Cr₂NO₃
The number in the subscript of the chemical formula of the given element signifies the number of atom or ions of the given element. In this regard, based on the chemical formula written for chromium (II) nitrate, the number of chromium ions would have to be 2.
<em>Answer: 2</em>
Answer: 1 mol C8H18 produces 9 mol H2O
Explanation: reaction : C8H18 + 12.5 O2 ⇒ 8 CO2 + 9 H2O
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