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Bingel [31]
3 years ago
14

A light bulb contains 0.0560 g of argon gas with a pressure of 1.34 atm at 26.0 c. The light bulb is then turned on and, after a

period of time, the temperature rises to 179c. Calculate the final pressure the light bulb
Chemistry
1 answer:
jenyasd209 [6]3 years ago
7 0

Answer:

Final pressure of light bulb is 2.03 atm.

Explanation:

Given data:

Initial pressure = 1.34 atm

initial temperature = 26 °C

Finial temperature = 179 °C

Final pressure = ?

Formula:

P1/T1 = P2/T2

Solution:

First of all we will convert the °C into kelvin.

179 +273 = 452 K

26 +273 = 299 K

P2 = P1×T2/T1

P2 = 1.34 atm . 452 K / 299 K

P2 = 605.68 atm/ 299

P2 = 2.03 atm

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How many grams of iron can be made with 21.5g of Fe2O3
SIZIF [17.4K]

The mass (in grams) of iron, Fe that can be made from 21.5 g of Fe₂O₃ is 15.04 g

We'll begin by writing the balanced equation for the reaction. This is given below:

2Fe₂O₃ -> 4Fe + 3O₂

  • Molar mass of Fe₂O₃ = 159.7 g/mol
  • Mass of Fe₂O₃ from the balanced equation = 2 × 159.7 = 319.4 g
  • Molar mass of Fe = 55.85 g/mol
  • Mass of Fe from the balanced equation = 4 × 55.85 = 223.4 g

From the balanced equation above,

319.4 g of Fe₂O₃ decomposed to produce 223.4 g of Fe

<h3>How to determine the mass of iron, Fe produced</h3>

From the balanced equation above,

319.4 g of Fe₂O₃ decomposed to produce 223.4 g of Fe

Therefore,

21.5 g of Fe₂O₃ will decompose to produce = (21.5 × 223.4) / 319.4 = 15.04 g of Fe

Thus, 15.04 g of Fe were produced.

Learn more about stoichiometry:

brainly.com/question/9526265

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