Chemistry Chapter 5 Quiz

<p>$CH_4$ (B)</p> Signup and view all the answers

<p>22.4 L (B)</p> Signup and view all the answers

<p>The uncertainty in its velocity is zero (D)</p> Signup and view all the answers

<p>22.4 L $CH_4$ at STP (C)</p> Signup and view all the answers

<p>At an angle of 45° from the x and y axis (D)</p> Signup and view all the answers

<p>1.0 mole of $O_2$ (A)</p> Signup and view all the answers

<p>4 mole P atom (C)</p> Signup and view all the answers

One mole of P4 contains 4 P atoms.

1 mole of O₂ weighs 32 grams.

22.4 L of any gas at STP equals 1 mole of gas.

The product of position uncertainty and momentum uncertainty is ≥ ħ/2.

4 g of Helium occupies 22.4 L at STP.

Vapor density of a gas is half of its molar mass.

49 g of H₂SO₄ contains 1 mole of S atom.

Gas having vapor density double O₂ could be SO₂.

6 x 10²³ molecules of Na2CO3 weigh 106 g.

The vapor density and weight help determine its identity.

SO₂ has a different vapor density compared to O₂.

CO₂ has a vapor density based on its molar mass.

6 x 10²³ molecules represents 1 mole of substance.

Highest probability of finding an electron in d_{xy} is at 45°.

All ideal gases occupy 22.4 L at STP per mole.

Maximum certainty in position means minimum uncertainty in velocity.

Gases behave predictably under standard temperature and pressure.

High vapor density means heavier molecular weight.

SO₃'s vapor density suggests a high molecular mass.

Atomic weight is crucial for calculating gas moles or weight.

STP is standard conditions used for gas calculations.

To find weight, multiply moles by molar mass.

Use formulas to determine the moles in compounds.

Gases expand to fill their containers and have low density.

Applies to high-energy particles and atomic scale measurements.