Answer:
Explanation:
The pressure is constant, so we can use Charles' Law.
Data:
V₁ = 1.92 × 10³ L; T₁ = 20 °C
V₂ = ?; T₂ = 68 °C
Calculations:
(a) Convert temperatures to kelvins
T₁ = (20 + 273.15) K = 293.15 K
T₂ = (68 + 273.15) K = 341.15 K
(b) Calculate the volume
The new volume of the gas is .
The STP stands for standard temperature and pressure which means in a condition where the temperature is 273.15K and the pressure is 0.986atm. In STP, an ideal gas will have a volume 22.4 liters for every mol of gas. Then, the amount of molecule of the <span>33.6 l of chlorine gas (Cl2) would be:
volume of gas/ number of mol= 22.4l/mol
</span>33.6l/ number of mol= 22.4l/mol
<span>number of mol= 33.6l / (22.4 liters/mol)= 1.5 moles
The mass of the gas would be: 1.5 moles * </span><span>70.906 </span>g/mol= 106.359 grams
Answer is: <span>the objects potential energy is 24500 J.
</span>m(object) = 50 kg.
h(object) = 50 m.
g = 9,8 m/s².
E(object) = m·g·h.
E(object) = 50 kg · 9,8 m/s² · 50 m.
E(object) = 24500 N·m = 24500 J = 24,5 kJ.
g - <span>the acceleration of free fall.
mg - </span><span>weight of the object.</span>
Answer:
0.036 g
Explanation:
<em>0.036 g of water should be produced.</em>
From the equation of reaction, 1 mole of HCl requires 1 mole of NaOH in order to produce 1 mole of H2O.
20 mL of 0.10 M HCl contains 20/1000 x 0.10 = 0.002 moles of HCl
46 grams of NaOH contains 46/40 = 1.15 moles of NaOH
<em>It thus means that the HCl is a limiting reagent in the reaction.</em>
From the equation:
1 mole HCl will produce 1 mole of H2O.
0.002 HCl with therefore produce 0.002 x 1/1 = 0.002 mole of H2O
<em>Mass of water produced = mole x molar mass</em>
0.002 x 18 = 0.036 g.
Hence, 0.036 g of water would be produced.
