Which of the following would most likely act as a Bronsted-Lowry acid?

How does an acid–base indicator react when placed in an acidic solution?It changes color.
It dissolves.
It increases the pH of the solution.
It releases hydroxide ions.

A scientist is performing an experiment on a powder. Which of the following is a sign that a chemical change has definitely occurred during his experiment?The powder catches on fire.
The powder releases bubbles.
The powder heats up.
The powder breaks apart into smaller particles.

Which statement best describes the effect of low ionization energies and low electronegativities on metallic bonding? a. The valence electrons are easily delocalized.
b. The valence electrons stay in a single orbital.
c. The valence electrons break free of the crystals.
d. The valence electrons move closer to the nuclei.

Magnesium and nitrogen react in a combination reaction to produce magnesium nitride: 3 Mg + N2 → Mg3N2 In a particular experiment, a 9.27-g sample of N2 reacts completely. The mass of Mg consumed is __________ g.

The element carbon, nitrogen, and oxygen are all part of the same?

Are these answers correct?1. A gas occupies 30 L at 760 mm Hg. What is its volume at 350 mm Hg?

P1*V1 = P2*V2

760 mm Hg *30 L = 350 mm Hg * V2

V2 = 22800 mm Hg*L/350 mm Hg

V2 = about 65.14 L


2. A gas occupies 500 mL at 1 atm. What is its pressure if the volume becomes 1500 mL?

P1*V1 = P2*V2

1 atm*500 mL = P2*1500 mL

500 atm*mL/1500 mL = P2

P2 = 1/3 atm


3. If a gas occupies 250 mL at 25°C, what will its volume be at 57°C?

25°C + 273 = 298°K; 57°C + 273 = 330°K

V1/T1 = V2/T2

250 mL/298°K = V2/330°K

0.84 mL/k*330°K = V2

V2 = about 276.85 mL

4. What was the original temperature of a 2 L sample of gas if it initially had the volume 5 L at 27°C?

27°C + 273 = 298°K

V1/T1 = V2/T2

5 L/298°K = 2 L/T2

2 L/(0.017 L/K)= T2

T2 = 119.2°K = -153.8°C

5. At what pressure would 100 mL of a gas be found if it began at 500 mL at 2.5 atm?

P1*V1 = P2*V2

2.5 atm*500 mL = P2*100 mL

125 atm*mL/100 mL = P2

P2 = 1.25 atm

6. What is the volume of a gas at 275 mm Hg if it occupied 750 mL at 1000 mm Hg?

P1*V1 = P2*V2

1000 mm Hg*750 mL = 275 mm Hg*V2

750000 mm Hg*mL/275 mm Hg = V2

V2 = about 2727. 27 mL

7. A gas occupies 60 L at 250°K and 1 atm. What is its volume at 250°C and 1.5 atm?

250°C + 273 = 523°K

P1*V1/T1 = P2*V2/T2

1 atm*60 L/250°K = 1.5 atm*V2/523°K

0.24 (atm*L/K)*523°K = 1.5 atm*V2

125.52 (atm*L)/1.5 atm = V2

V2 = 83.68 L

8. What is the final temperature in Celsius of a gas occupying 3.25 L at 750 mm Hg if it occupied 2250 mL at 37°C and 600 mm Hg?

37°C + 273 = 310°K; 2250 mL = 2.25 L

P1*V1/T1 = P2*V2/T2

600 mm Hg*2.25 L/310°K = 750 mm Hg*3.25 L/T2

2437.35 mm Hg*L/ (4.35 mm Hg*L/K) = T2

T2 = 559.69°K
T2 = about 286.69°C