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garri49 [273]
3 years ago
6

Anyone know what the answer is?

Chemistry
2 answers:
malfutka [58]3 years ago
4 0
2 Ag2O = 4 Ag + 1 O2
Snowcat [4.5K]3 years ago
4 0
2AgO2 -> 4Ag + (1)O2
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A sample of gas contains 6.25 × 10-3 mol in a 500.0 mL flask at 265°C. What is the pressure of the gas in kilopascals? Which var
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55.9 kPa; Variables given = volume (V), moles (n), temperature (T)

We must calculate <em>p</em> from <em>V, n</em>, and <em>T</em>, so we use <em>the Ideal Gas Law</em>:

<em>pV = nRT</em>

Solve for <em>p</em>: <em>p = nRT/V</em>

R = 8.314 kPa.L.K^(-1).mol^(-1)

<em>T</em> = (265 + 273.15) K = 538.15 K

<em>V</em> = 500.0 mL = 0.5000 L

∴ <em>p</em> = [6.25 x 10^(-3) mol x 8.314 kPa·L·K^(-1)·mol^(-1) x 538.15 K]/(0.5000 L) = 55.9 kPa

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3 years ago
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3 years ago
Can someone please help me with the correct formula for this?
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I'm not sure if you want the molecular formula or the condensed structure, but I will give you both.

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You have 2 carbons (C₂), 4 hydrogens (H₄), and 1 oxygen (O).  The molecular formula will be C₂H₄O.

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