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nlexa [21]
3 years ago
5

two substances react and the mass is recorded.The mass of the products does not equal the mass of the reactants .Which is the be

st explaination for the different masses?
Chemistry
1 answer:
Dovator [93]3 years ago
8 0
Mass can’t be destroyed. So since not all the mass was found in the products, that simply means that it was lost to the environment. For example, let’s say hydrogen and oxygen are the reactants and we get water in the product. Now that oxygen could have reacted with something else that we didn’t take into account when measuring the mass of the H2O released.

Tldr, some of the reactants were lost to the surroundings
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Consider 4.00 L of a gas at 365 mmHg and 20. ∘C . If the container is compressed to 2.80 L and the temperature is increased to 3
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This is an exercise in<u> the General Combined Gas Law</u>.

To start solving this exercise, we obtain the following data:

<h3>Data:</h3>
  • V₁ = 4.00 l
  • P₁ = 365 mmHg
  • T₁ = 20 °C + 273 = 293 K
  • V₂ = 2,80 l
  • T₂ = 30 °C + 273 = 303 K
  • P₂ = ¿?

We apply the following formula:

  • P₁V₁T₂=P₂V₂T₁     ⇒  General formula

Where:

  • P₁=Initial pressure
  • V₁=Initial volume
  • T₂=end temperature
  • P₂=end pressure
  • T₂=end temperature
  • V₁=Initial temperature

We clear for final pressure (P2)

\large\displaystyle\text{$\begin{gathered}\sf P_{2}=\frac{P_{1}V_{1}T_{2}}{V_{2}T_{1}} \ \ \to \ \ \ Formula \end{gathered}$}

We substitute our data into the formula:

\large\displaystyle\text{$\begin{gathered}\sf P_{2}=\frac{(365 \ mmHg)(4.00 \not{l})(303 \not{K})}{(2.80 \not{l})(293\not{K})}  \end{gathered}$}

\large\displaystyle\text{$\begin{gathered}\sf P_{2}=\frac{442380 \ mmHg}{ 820.4 }  \end{gathered}$}

\boxed{\large\displaystyle\text{$\begin{gathered}\sf P_{2}=539.224 \ mmHg \end{gathered}$}}

Answer: The new canister pressure is 539.224 mmHg.

<h2>{ Pisces04 }</h2>
6 0
1 year ago
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