ank, V = 2 m³, ideal gas P = 2 MPa, T = 400 K. T increases 80 K, V constant. P?

Question and answer

P2 = P1 (T2/T1) P2 = 2×10^6 × (480/400) P2 = 2.4×10^6 Pa

Question

Asked 25 days ago|2/10/2026 12:54:34 PM

Updated 25 days ago|2/10/2026 1:54:45 PM

2 Answers/Comments

Get an answer

Search for an answer or ask Weegy.

New answers

Rating

cruz30

P2 = P1 (T2/T1)
P2 = 2×10^6 × (480/400)
P2 = 2.4×10^6 Pa

Added 25 days ago|2/10/2026 1:39:29 PM

This answer has been confirmed as correct and helpful.

Salas1987

T2 = T1 + T = 400 K + 80 K = 480 K
P1/T1 = P2/T2
P2 = P1 * (T2/T1)
P2 = (2 x 10^6 Pa) * (480 K / 400 K)
P2 = (2 x 10^6 Pa) * 1.2
P2 = 2.4 x 10^6 Pa.

Therefore, the final pressure (P2) is 2.4 MPa.

Added 25 days ago|2/10/2026 1:54:45 PM

Comments

There are no comments.

Add an answer or comment

Questions asked by the same visitor

Calculate the temperature at which 50% of N O dissociates into NO , given H° = 57 kJ/mol and S° = 175 J/mol·K.

(More)

Question

Not Answered

Updated 26 days ago|2/9/2026 9:45:27 AM

1 Answer/Comment

cruz30

Given:
H° = 57 kJ/mol = 57000 J/mol, S° = 175 J/mol·K
50% dissociation - K = 1
Gibbs free energy: G° = H° - T S° = -RT ln K
ln K = 0 - G° = 0 - T = H° / S° = 57000 / 175 = 325.7 K
Answer: T = 326 K

Added 26 days ago|2/9/2026 9:45:27 AM

This answer has been confirmed as correct and helpful.

Determine the concentration of OH in a solution prepared by dissolving 0.05 mol of K CO in 500 mL of water.

(More)

Question

Not Answered

Updated 26 days ago|2/9/2026 9:45:53 AM

1 Answer/Comment

cruz30

Given:
n = 0.05 mol, V = 0.5 L
Concentration: [OH ] = n / V = 0.05 / 0.5 = 0.1 M
Answer: [OH ] = 0.1 M

Added 26 days ago|2/9/2026 9:45:53 AM

This answer has been confirmed as correct and helpful.

Calculate the standard Gibbs free energy of formation for SO from S and O using H°f and S° values.

(More)

Question

Not Answered

Updated 26 days ago|2/9/2026 9:46:21 AM

1 Answer/Comment

cruz30

Given:
Reaction: S + 1/2 O - SO
H°f (SO) = 0 kJ/mol (assume known), S° values: S(S) = S1, S(O ) = S2, S(SO) = S3
G°f = H°f - T S°
S° = S_products - S_reactants = S(SO) - [S(S) + 0.5 S(O )]
G°f = H°f - T × S°
Answer: G°f = H°f - T × (S(SO) - S(S) - 0.5 S(O ))

Added 26 days ago|2/9/2026 9:46:21 AM

This answer has been confirmed as correct and helpful.

Determine the fraction of carbon atoms in C H O that are sp³ hybridized.

(More)

Question

Not Answered

Updated 26 days ago|2/9/2026 9:53:07 AM

1 Answer/Comment

cruz30

Given: C H O
Identify hybridization:
- Total C = 4
- Structure (possible): CH –CH –CH –OH or similar
- sp³ C: all C bonded to 4 atoms - 3 C are sp³, 1 C may be sp² if in carbonyl (depends on structure)
Assume most common: C H O is an alcohol (CH -CH -CH –-OH) - all C sp³
Fraction = sp³ C / total C = 4 / 4 = 1
Answer: Fraction = 1 (100%)

Added 26 days ago|2/9/2026 9:53:07 AM

This answer has been confirmed as correct and helpful.

A reaction A B follows the Arrhenius equation. Given k = 0.05 s ¹ at 300 K and k = 0.15 s ¹ at 350 K, calculate the activation energy.

(More)

Question

Not Answered

Updated 26 days ago|2/9/2026 9:52:12 AM

1 Answer/Comment

cruz30

Given:
k1 = 0.05 s ¹ at T1 = 300 K
k2 = 0.15 s ¹ at T2 = 350 K
Arrhenius: ln(k2/k1) = Ea/R (1/T1 - 1/T2)
ln(0.15/0.05) = ln 3 = 1.0986
1/T1 - 1/T2 = 1/300 - 1/350 = 0.00047619 K ¹
Ea = R × ln(k2/k1) / (1/T1 - 1/T2) = 8.314 × 1.0986 / 0.00047619 = 19176 J = 19.2 kJ/mol
Answer: Ea = 19.2 kJ/mol

Added 26 days ago|2/9/2026 9:52:12 AM

This answer has been confirmed as correct and helpful.

40,356,863

questions answered