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FinnZ [79.3K]
3 years ago
12

If 50.75 g of a gas occupies 10.0 l at stp, 129.3 g of the gas will occupy __________ l at stp.

Chemistry
2 answers:
Rom4ik [11]3 years ago
6 0
Use PV = mRT/M and solve for R. R = PVM/RT. Since you have the same gas under two sets of conditions then you can write 
<span>P1V1M1/m1T1 = P2V2M2/m2T2 </span>
<span>Since P, M and T are constant, the equation becomes </span>
<span>V1/m1 = V2/m2 </span>
<span>Now plug in your values and solve for V2</span>
Semenov [28]3 years ago
4 0

Answer: 25.5 L

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 Liters at STP and contains avogadro's number 6.023\times 10^{23} of particles.

We are given:

50.75 g of a gas occupies = 10.0 L at STP

Thus 129.3 g  of a gas occupies =\frac{10}{50.75}\times 129.3=25.5L at STP

Thus 129.3 g of gas will occupy 25.5 L at STP.

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Answer:

Single-Replacement Reaction

General Formulas and Concepts:

<u>Chemistry - Reactions</u>

  • Synthesis Reactions: A + B → AB
  • Decomposition Reactions: AB → A + B
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  • Double-Replacement Reactions: AB + CD → AD + BC

Explanation:

<u>Step 1: Define RxN</u>

Mg + H₂SO₄ → MgSO₄ + H₂

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

Mg + H₂SO₄ → MgSO₄ + H₂

Single-Replacement Reaction A + BC → AB + C

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Which of the following gives the net ionic reaction for the reaction used in this experiment?
CaHeK987 [17]

Answer: Option (d) is the correct answer.

Explanation:

The given reaction will be as follows.

       Ba(OH)_{2}(aq) + H_{2}SO_{4}(aq) \rightarrow BaSO_{4}(s) + 2H_{2}O(l)

In the ionic form, the equation will be as follows.

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Hence, for the net ionic equation we need to add both equation (1) and (2). Therefore, the net ionic equation will be as follows.

     Ba^{2+}(aq) + SO^{2-}_{4}(aq) + H^{+}(aq) + OH^{-}(aq) \rightarrow BaSO_{4}(s) + H_{2}O(l)        

Now, balancing the atoms on both the sides we get the net ionic equation as follows.

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chubhunter [2.5K]

Answer:

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455 grams mercury              1 mL
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