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Pavlova-9 [17]
2 years ago
15

What is the mass of 22.4L of H2 at stp

Chemistry
1 answer:
bazaltina [42]2 years ago
5 0

Answer:

2.02 g H₂

General Formulas and Concepts:

<u>Chemistry - Atomic Structure</u>

  • Reading a Periodic Table
  • Using Dimensional Analysis
  • STP (Standard Conditions for Temperature and Pressure) = 22.4 L per mole at 1 atm, 273 K

Explanation:

<u>Step 1: Define</u>

22.4 L H₂ at STP

<u>Step 2: Identify Conversions</u>

STP - 22.4 L / mol

Molar Mass of H - 1.01 g/mol

Molar Mass of H₂ - 2(1.01) = 2.02 g/mol

<u />

<u>Step 3: Convert</u>

<u />22.4 \ L \ H_2(\frac{1 \ mol \ H_2}{22.4 \ L \ H_2} )(\frac{2.02 \ g \ H_2}{1 \ mol \ H_2} ) = 2.02 g H₂

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Answer:

Kp=3.07x10^6

Explanation:

Hello,

In this case, by knowing the given reference reactions, one could rearrange them as follows:

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N_2(g) + 2O_2(g) \leftrightarrow 2NO_2(g);Kp_3=(8.4x10^{-7})^2=7.056x10^{-13}

Subsequently, to obtain the main reaction, we add the aforementioned reference rearranged reactions as shown below (just as reference):

2NO(g)+N_2(g)+2O_2\leftrightarrow 2NO_2(g)+N_2+O_2

Consequently, the equilibrium constant is computed as:

Kp=\frac{[N_2][O_2]}{[NO]^2} * \frac{[NO_2]^2}{[N_2][O_2]^2} =Kp_2*Kp_3=4.35x10^{18}*7.056x10^{-13}=3.07x10^6

Best regards.

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A wildfire can destroy thousands of acres of forest. Explain two positive effects and two negative effects that a wildfire can h
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Explanation:

Wildfires destroy forests that are great carbon sinks. This means that large amount of carbon dioxide are released back into the atmosphere. Carbon dioxide is a greenhouse gas and this will contribute to global warming.

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3 years ago
to find the density of stopper I weighted it and found its mass to 4.8g. After that I filled a graduated cylinder with 32.1mL of
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Answer:

0.68g/ml

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