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Mandarinka [93]
1 year ago
7

A sample of helium gas inside a closed but flexible container occupies a volume of 355mL at 23°C. If the pressure is held consta

nt, to what temperature must the He be raised to cause the container to expand to a final volume of 1.50 L?
Chemistry
1 answer:
guapka [62]1 year ago
6 0

Answer:

978.19° C

Explanation:

P1V1/T1 =P2V2/T2     Since the pressure is constant, this can be written as

V1/T1 = V2/T2      RE-ARRANGE TO

V2 *  T1/V1   = T2       Note:  T must be in Kelvin!!

1.5 L  *  (273.15 + 23)  / (.355 L ) = T2 = 1251.338 K  =978.19 C

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If a reaction generated 3.5 g of H2O how many moles of water were formed?
professor190 [17]

Answer:

0.19 mol H₂O

General Formulas and Concepts:

<u>Chem</u>

  • Reading a Periodic Table
  • Using Dimensional Analysis

Explanation:

<u>Step 1: Define</u>

Given: 3.5 g H₂O from RxN

<u>Step 2: Define conversions</u>

Molar Mass of H - 1.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of H₂O - 2(1.01) + 16.00 = 18.02 g/mol

<u>Step 3: Convert</u>

<u />3.5 \ g \ H_2O(\frac{1 \ mol \ H_2O}{18.02 \ g \ H_2O} ) = 0.194229 mol H₂O

<u>Step 4: Check</u>

<em>We are given 2 sig figs. Follow sig fig rules.</em>

0.194229 mol H₂O ≈ 0.19 mol H₂O

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