Due to increase in temperature will decreases both solubility and rate of the solute.
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<span>How many molecules of H20 are in 2.0 moles
</span>
12.044*10^23 or 6.022⋅1023 <span>atoms</span>
The ideal gas law is P1V1/T1 = P2V2/T2. STP means the temperature is 273 K and pressure is 101.3 kPa. According to this formula, the new volume V2=2.15*58*273/(298*101.3) = 1.13 L.
Formula Equation of this Neutralization reaction is,
RbOH₍aq₎<span> + HClO</span>₄₍aq₎ → RbClO₄₍aq₎<span> + H</span>₂O₍l₎
<span>Overall Ionic Equation is as follow,
</span> Rb⁺₍aq₎ + OH⁻₍aq₎ + H₃O⁺₍aq₎ + ClO₄⁻₍aq₎ → Rb⁺₍aq₎ + ClO₄⁻₍aq₎ + 2H₂O₍l₎
And <span>Net Ionic Equation is as follow,
</span><span> H</span>₃O⁺₍aq₎<span> + OH</span>⁻₍aq₎ →<span> 2H</span>₂O₍l₎
Answer:
Explanation:
no. of moles of butane = 5.87g / 58.124 = 0.1009mol
since O2 is excess, limiting reagent is butane
from the equation, 2 moles of butane will reacted to produce water = 10 moles
therefore, 0.1009 moles of butane produced water = (0.1009 x 5) = 0.5050 moles
Weight of H2O formed = 0.5050 x 18.015 = 9.10 grams
